Question

(c) Potassium hydroxide reacts completely with sulfuric acid according to the equation:
H2SO4(aq) + 2KOH(aq) K2SO4(aq) + 2H2O(l)
0.95 g of potassium hydroxide were dissolved in water and made up to 250 cm3 of solution. 25 cm3 samples of this solution were titrated against sulfuric acid (H2SO4) solution. The mean volume (titre) of sulfuric acid required for complete reaction was 15.00 cm3.
(i) Find the molar concentration of the prepared solution of potassium hydroxide. Complete the calculation given below:
Relative Molecular Mass (RMM) of KOH = 56 .1g/mole/250
= 1.58cm3……………………… (1 mark)
No. of moles of KOH in 250 cm3 =
= ………………………… (1 mark)
 molar concentration of KOH =
(Include units in your answer) = ………………………… (1 mark)





Continued…..

(ii) Find the molar concentration of the sulfuric acid from the titration result:
Complete the calculation given below:
No. of moles of KOH in 25.00 cm3 =
= ………………………… (1 mark)
 no. of moles H2SO4 in 15.00 cm3 =
= ………………………… (1 mark)
 molar concentration of H2SO4 =
(Include units in your answer) = ………………………… (2 marks)

(Total 10 marks)

Answer 1

Answer:

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