Category: Chemistry

Calculate the mass of sodium ethanoate salt ( Mr of 82 ) that would need to be added to 600 cm³ of 0.300 mol dm^-3 ethanoic acid solution to produce a pH of 5.00

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the mass of sodium methanoate salt ( Mr of 68 ) that would need to be added to 50.0 cm³ of 0.110 mol dm^-3 methanoic acid solution to produce a pH of 4.75

The acid dissociation constant, Ka, for methanoic acid is 1.78 x 10^-4 mol dm^-3

Calculate the mass of lithium ethanoate salt ( Mr of 66.0 ) that would need to be added to 45.0 cm³ of 0.200 mol dm^-3 ethanoic acid solution to produce a pH of 4.54

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the mass of sodium ethanoate salt ( Mr of 82 ) that would need to be added to 50.0 cm³ of 0.100 mol dm^-3 ethanoic acid solution to produce a pH of 5.20

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution produced when 0.100 g of sodium ethanoate salt ( Mr of 82 )is added to 50.0 cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5mol dm^-3

Calculate the pH of a solution produced when 0.458 g of potassium cyanide salt ( Mr of 65.1 )is added to 94.0 cm³ of 0.100 mol dm^-3 hydrocyanic acid solution.

The acid dissociation constant, Ka, for hydrocyanic acid is 6.20 x 10^-10mol dm^-3

Calculate the pH of a solution produced when 1.00 g of sodium phenoxide salt ( Mr of 116.1 )is added to 75.0 cm³ of 0.300 mol dm^-3 phenol solution.

The acid dissociation constant, Ka, for phenol is 1.0 x 10^-10mol dm^-3

Calculate the pH of a solution produced when 75.0 cm³ of 0.300 mol dm^-3 lithium hydroxide solution has been added to 50.0cm³ of 0.500 mol dm^-3 hydrofluoric acid solution.

The acid dissociation constant, Ka, for hydrofluoric acid is 6.60 x 10^-4 mol dm^-3

Calculate the pH of a solution produced when 20.0 cm³ of 0.200 mol dm^-3 potassium hydroxide solution has been added to 80.0cm³ of 0.100 mol dm^-3 methanoic acid solution.

The acid dissociation constant, Ka, for methanoic acid is 1.78 x 10^-4 mol dm^-3

Calculate the pH of a solution produced when 20.0 cm³ of 0.200 mol dm^-3 potassium hydroxide solution has been added to 90.0cm³ of 0.100 mol dm^-3 methanoic acid solution.

The acid dissociation constant, Ka, for methanoic acid is 1.78 x 10^-4 mol dm^-3

Calculate the mass of sodium phenoxide salt ( Mr of 116.1 ) that would need to be added to 75.0 cm³of 0.300 mol dm^-3 phenol solution to produce a pH of 9.50

The acid dissociation constant, Ka, for phenol is 1.00 x 10^-10 mol dm^-3

Calculate the pH of a solution produced when 0.582 g of lithium fluoride salt ( Mr of 25.9 )is added to 50.0 cm³ of 0.500 mol dm^-3 hydrofluoric acid solution.

The acid dissociation constant, Ka, for hydrofluoric acid is 6.60 x 10^-4mol dm^-3

Calculate the pH of a solution produced when 3.080 g of potassium methanoate salt ( Mr of 84.1 )is added to 80.0 cm³ of 0.900 mol dm^-3 methanoic acid solution.

The acid dissociation constant, Ka, for methanoic acid is 1.78 x 10^-4mol dm^-3

Calculate the pH of a solution produced when 1.00 g of potassium methanoate salt ( Mr of 84.1 )is added to 90.0 cm³ of 0.100 mol dm^-3 methanoic acid solution.

The acid dissociation constant, Ka, for methanoic acid is 1.78 x 10^-4mol dm^-3

Calculate the pH of a solution produced when 49.0 cm³ of 0.100 mol dm^-3 sodium hydroxide solution has been added to 50.0cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution produced when 40.0 cm³ of 0.100 mol dm^-3 sodium hydroxide solution has been added to 50.0cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution produced when 25.0 cm³ of 0.100 mol dm^-3 sodium hydroxide solution has been added to 50.0cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution produced when 20.0 cm³ of 0.100 mol dm^-3 sodium hydroxide solution has been added to 50.0cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution produced when 10.0 cm³ 0.100 mol dm^-3 sodium hydroxide solution has been added to 50.0cm³ of 0.100 mol dm^-3 ethanoic acid solution.

The acid dissociation constant, Ka, for ethanoic acid is 1.70 x 10^-5 mol dm^-3

Calculate the mass of potassium cyanide salt ( Mr of 65.1 ) that would need to be added to 94.0 cm³of 0.100 mol dm^-3 hydrocyanic acid solution to produce a pH of 8.51

The acid dissociation constant, Ka, for hydrocyanic acid is 6.20 x 10^-10 mol dm^-3

Hydrofluoric acid is a weak acid with a pKa value of 3.18

Calculate the concentration of a solution of hydrofluoric acid that would produce a pH of 2.11

Ethanoic acid is a weak acid with a pKa value of 4.77

Calculate the concentration of a solution of ethanoic acid that would produce a pH of 2.43

Nitrous acid (nitric (III) acid) is a weak acid with a pKa value of 3.25

Calculate the concentraion of a solution of nitrous acid (nitric (III) acid) that would produce a pH of 1.62

A solution of hydrocyanic acid was found to have a pH of 4.37 when the concentraion of the hydrocyanic acid was 3.000 mol dm^-3

Calculate the value of Ka for hydrocyanic acid

A solution of phenol was found to have a pH of 5.01 when the concentraion of the phenol was 0.950 mol dm^-3

Calculate the value of Ka for phenol

A solution of benzoic acid was found to have a pH of 2.27 when the concentration of the benzoic acid was 0.450 mol dm^-3

Calculate the value of Ka for benzoic acid

Hydrofluoric acid is a weak acid with a pKa value of 3.18

Calculate the pH of a solution of hydrofluoric acid when it is in a concentration of 0.450 mol dm^-3

Methanoic acid is a weak acid with a pKa value of 3.75

Calculate the pH of a solution of methanoic acid when it is in a concentration of 0.650 mol dm^-3

Propanoic acid is a weak acid with a pKa value of 4.87

Calculate the pH of a solution of propanoic acid when it is in a concentration of 0.345 mol dm^-3

Ethanoic acid is a weak acid with a pKa value of 4.77

Calculate the pH of a solution of ethanoic acid when it is in a concentration of 0.250 mol dm^-3

Hydrofluoric acid is a weak acid with a Ka value of 6.60 x 10^-4 mol dm^-3

Calculate the concentration of a solution of hydrofluoric acid that would produce a pH of 2.05

Ethanoic acid is a weak acid with a Ka value of 1.70 x 10^-5 mol dm^-3

Calculate the concentration of a solution of ethanoic acid that would produce a pH of 2.51

Nitrous acid (nitric (III) acid) is a weak acid with a Ka value of 5.60x 10^-4 mol dm^-3

Calculate the concentration of a solution of nitrous acid (nitric (III) acid) that would produce a pH of 1.33

A solution of hydrocyanic acid was found to have a pH of 4.56 when the concentration of the hydrocyanic acid was 1.250 mol dm^-3

Calculate the value of Ka for hydrocyanic acid

A solution of phenol was found to have a pH of 4.87 when the concentraion of the phenol was 1.800 mol dm^-3

Calculate the value of Ka for phenol

A solution of benzoic acid was found to have a pH of 2.36 when the concentration of the benzoic acid was 0.300 mol dm^-3

Calculate the value of Ka for benzoic acid

Hydrofluoric acid is a weak acid with a Ka value of 6.60 x 10^-4 mol dm^-3

Calculate the pH of a solution of hydrofluoric acid when it is in a concentration of 0.300 mol dm^-3

Methanoic acid is a weak acid with a Ka value of 1.78 x 10^-4 mol dm^-3

Calculate the pH of a solution of methanoic acid when it is in a concentration of 0.100 mol dm^-3

Propanoic acid is a weak acid with a Ka value of 1.34 x 10^-5 mol dm^-3

Calculate the pH of a solution of propanoic acid when it is in a concentration of 0.100 mol dm^-3

Ethanoic acid is a weak acid with a Ka value of 1.70 x 10^-5 mol dm^-3

Calculate the pH of a solution of ethanoic acid when it is in a concentration of 0.100 mol dm^-3

Calculate the pH of a 0.0850 mol dm^-3 solution of nitric acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 1.00 x 10^-3 mol dm^-3 solution of barium hydroxide (Ba(OH)₂) solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0225 mol dm^-3 solution of barium hydroxide (Ba(OH)₂) solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.670 mol dm^-3 solution of potassium hydroxide solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.300 mol dm^-3 solution of sodium hydroxide solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 1.30 x 10^-3 mol dm^-3 solution of hydrobromic acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 1.89 x 10^-3 mol dm^-3 solution of hydroiodic acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig

Calculate the pH of a 0.0100 mol dm^-3 solution of sulfuric acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0750 mol dm^-3 solution of chloric (VII) acid (HClO₄). Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0850 mol dm-3 solution of nitric acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0300 mol dm^-3 solution of barium hydroxide (Ba(OH)₂) solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 2.30 x 10^-3 mol dm^-3 solution of barium hydroxide (Ba(OH)₂) solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig

Calculate the pH of a 0.0300 mol dm-3 solution of barium hydroxide (Ba(OH)2) solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.150 mol dm^-3 solution of potassium hydroxide solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.100 mol dm^-3 solution of sodium hydroxide solution. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 1.20 x 10^-3 mol dm^-3 solution of hydrobromic acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig

Calculate the pH of a 2.30 x 10^-3 mol dm^-3 solution of hydroiodic acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0750 mol dm^-3 solution of sulfuric acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a 0.0900 mol dm^-3 solution of chloric (VII) acid (HClO₄). Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig

Calculate the pH of a 0.100 mol dm^-3 solution of nitric acid. Assume that the acid fully dissociates in solution. Remember to give answer to 3 sig. fig.

Calculate the pH of a solution created by the addition of 25.0cm³ 0.350 mol dm^-3 nitric acid solution to 42.0 cm³ 0.150 mol dm^-3 barium hydroxide (Ba(OH)₂) solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 40.0cm³ 0.200 mol dm^-3 sulfuric acid solution to 90.0 cm³ 0.200 mol dm^-3 lithium hydroxide solution.

Remember to give your answer to 3 sig.fig

Calculate the pH of a solution created by the addition of 45.0cm³ 0.150 mol dm^-3 hydrochloric acid solution to 90.0 cm³ 0.200 mol dm^-3 sodium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 41.0cm³ 0.800 mol dm^-3 nitric acid solution to 45.0 cm³ 0.900 mol dm^-3 potassium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 99.9cm³ 0.250 mol dm^-3 barium hydroxide (Ba(OH)₂) solution to 100 cm³ 0.500 mol dm^-3 chloric (I) acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 30.0cm³ 0.100 mol dm^-3 potassium hydroxide solution to 40.0 cm³ 0.100 mol dm^-3 hydroiodic solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 38.0cm³ 0.150 mol dm^-3 barium hydroxide (Ba(OH)₂) solution to 60.0 cm³ 0.210 mol dm^-3 hydrochloric acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 80.0cm³ 0.300 mol dm^-3 sodium hydroxide solution to 200 cm³ 0.150 mol dm^-3 hydrochloric acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 15.0cm³ of 0.360 mol dm^-3 lithium hydroxide solution to 55.0 cm³ of 0.200 mol dm^-3 nitric acid solution.

Remember to give your answer to 3 sig.fig

Calculate the pH of a solution created by the addition of 99.9cm³ 0.100 mol dm^-3 sulfuric acid solution to 50.0 cm³ 0.200 mol dm^-3 barium hydroxide (Ba(OH)₂) solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 20.0cm³ 0.100 mol dm^-3 hydrochloric acid solution to 50.0 cm³ 0.100 mol dm^-3 potassium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 49.9cm³ 0.100 mol dm^-3 sulfuric acid solution to 25.0 cm³ 0.200 mol dm^-3 barium hydroxide (Ba(OH)₂) solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 25.0cm³ 0.350 mol dm^-3 hydrochloric acid solution to 30.0 cm³ 0.150 mol dm^-3 barium hydroxide (Ba(OH)₂) solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 28.0cm³ 0.100 mol dm^-3 sulfuric acid solution to 30.0 cm³ 0.200 mol dm^-3 lithium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 30.0cm³ 0.200 mol dm^-3 nitric acid solution to 70.0 cm³ 0.100 mol dm^-3 sodium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 20.0cm3 0.100 mol dm-3 hydrochloric acid solution to 50.0 cm3 0.100 mol dm-3 potassium hydroxide solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 49.0cm³ 0.250 mol dm^-3 barium hydroxide (Ba(OH)₂) solution to 100 cm³ 0.250 mol dm^-3 chloric (VII) acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 30.0cm³ 0.100 mol dm^-3 lithium hydroxide solution to 35.0 cm³ 0.100 mol dm^-3 hydrobromic acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 20.0cm³ 0.150 mol dm^-3 barium hydroxide (Ba(OH)₂) solution to 60.0 cm³ 0.200 mol dm^-3 hydrochloric acid solution.

Remember to give your answer to 3 sig.fig.

Calculate the pH of a solution created by the addition of 20.0cm³ 0.200 mol dm^-3 potassium hydroxide solution to 50.0 cm³ 0.100 mol dm^-3 nitric acid solution.

Remember to give your answer to 3 sig.fig.

By titration, it was found that an average titre of 9.90cm³ of 1.00 mol dm^-3 solution of potassium carbonate was required to just neutralise a 25.00 cm³ sample of sulfuric acid solution. Calculate the concentraion of the sulfuric acid solution.

The equation for the reaction is

K₂CO_3(aq)+H₂SO_4(aq)=>K₂SO_4(aq)+H₂O_(aq)+CO_2(g)

By titration, it was found that an average titre of 19.95cm³ of 0.180 mol dm^-3 solution of nitric acid was required to just neutralise a 10.00 cm³ sample of sodium carbonate solution. Calculate the concentraion of the sodium carbonate solution.

The equation for the reaction is

2HNO_3(aq)+Na₂CO_3(aq)=>2NaNO_3(aq)+H₂O_(aq)+CO_2(g)

By titration, it was found that an average titre of 28.05cm³ of 0.100 mol dm^-3 solution of potassium hydroxide was required to just neutralise a 25.00 cm³ sample of phosphoric acid solution. Calculate the concentraion of the phosphoric acid solution.

The equation for the reaction is

3KOH_(aq)+H₃PO_4(aq)=>K₃PO_4(aq)+3H₂O_(aq)

By titration, it was found that an average titre of 21.25cm³ of 2.450 mol dm^-3 solution of sulfuric acid was required to just neutralise a 10.00 cm³ sample of barium hydroxide solution. Calculate the concentraion of the barium hydroxide solution.

The equation for the reaction is

H₂SO_4(aq)+Ba(OH)_2(aq)=>BaSO_4(aq)+2H₂O_(aq)

By titration, it was found that an average titre of 31.40cm³ of 0.200 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 25.00 cm³ sample of barium hydroxide solution. Calculate the concentraion of the barium hydroxide solution.

The equation for the reaction is

Ba(OH)_2(aq)+2HCl_(aq)=>BaCl_2(aq)+2H₂O_(aq)

By titration, it was found that an average titre of 21.30cm³ of 0.100 mol dm^-3 solution of sulfuric acid was required to just neutralise a 25.00 cm³ sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

2KOH_(aq)+H₂SO_4(aq)=>K₂SO_4(aq)+H₂O_(aq)

By titration, it was found that an average titre of 16.25cm³ of 0.500 mol dm^-3 solution of sulfuric acid was required to just neutralise a 10.00 cm³ sample of sodium hydroxide solution. Calculate the concentraion of the sodium hydroxide solution.

The equation for the reaction is

2NaOH_(aq)+H₂SO_4(aq)=>Na₂SO_4(aq)+H₂O_(aq)

By titration, it was found that an average titre of 19.75cm³ of 0.200 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 10.00 cm³ sample of lithium hydroxide solution. Calculate the concentraion of the lithium hydroxide solution.

The equation for the reaction is

LiOH_(aq)+HCl_(aq)=>LiCl_(aq)+H₂O_(aq)

By titration, it was found that an average titre of 25.00cm³ of 1.75 mol dm^-3 solution of nitric acid was required to just neutralise a 50.00 cm³ sample of potassium hydroxide solution. Calculate the concentraion of the potassium hydroxide solution.

The equation for the reaction is

KOH_(aq)+HNO_3(aq)=>KNO_3(aq)+H₂O_(aq)

By titration, it was found that an average titre of 20.00cm³ of 0.150 mol dm^-3 solution of hydrochloric acid was required to just neutralise a 10.00 cm³ sample of sodium hydroxide solution. Calculate the concentraion of the sodium hydroxide solution.

The equation for the reaction is

NaOH_(aq)+HCl_(aq)=>NaCl_(aq)+H₂O_(aq)

16.1g of citric acid monohydrate (C₆H₈O₇.H₂O), a tribasic acid, was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

10.0cm³ samples were titrated against potassium hydroxide solution of concentraion 0.500 mol dm^-3.

A mean titre of 18.10cm³ of potassium hydroxide solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

1.88g of adipic acid (C₆H₁₀O₄), a dibasic acid, was dissolved in deionised water and made up to 100cm³ in a volumetric flask.

10.0cm³ samples were titrated against sodium hydroxide solution of concentraion 0.100 mol dm^-3.

A mean titre of 24.50cm³ of sodium hydroxide solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!

2.49g of potassium hydroxide was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

20.0cm³ samples were titrated against hydrochloric acid solution of concentraion 0.150 mol dm^-3.

A mean titre of 21.90cm³ of hydrochloric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

1.98g of lithium carbonate was dissolved in deionised water and made up to 100cm³ in a volumetric flask.

25.0cm³ samples were titrated against hydrochloric acid solution of concentraion 0.500 mol dm^-3.

A mean titre of 25.35cm³ of hydrochloric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

1g of sodium hydroxide was dissolved in deionised water and made up to 100cm³ in a volumetric flask.

25.0cm³ samples were titrated against nitric acid solution of concentraion 0.200 mol dm^-3.

A mean titre of 28.25cm³ of nitric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

4.95g of potassium hydrogencarbonate was dissolved in deionised water and made up to 100cm³ in a volumetric flask.

10.0cm³ samples were titrated against sulfuric acid solution of concentraion 0.100 mol dm^-3.

A mean titre of 22.05cm³ of sulfuric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

2.81g of sodium carbonate was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

25.0cm³ samples were titrated against hydrochloric acid solution of concentraion 0.250 mol dm^-3.

A mean titre of 20.80cm³ of hydrochloric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

1.56g of lithium hydroxide was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

25.0cm³ samples were titrated against sulfuric acid solution of concentraion 0.100 mol dm^-3.

A mean titre of 23.20cm³ of sulfuric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

2.5g of potassium hydroxide was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

25.0cm³ samples were titrated against nitric acid solution of concentraion 0.150 mol dm^-3.

A mean titre of 18.15cm³ of nitric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)

1g of sodium hydroxide was dissolved in deionised water and made up to 250cm³ in a volumetric flask.

25.0cm³ samples were titrated against hydrochloric acid solution of concentraion 0.100 mol dm^-3.

A mean titre of 22.50cm³ of hydrochloric acid solution was obtained.

Calculate the percentage purity, by mass, of the original solid. (Don't include the % symbol and give answer to 1 decimal place!)