Question

23. Write a complete ionic and net-ionic equation for the following reaction. K2CO3(aq) + H2SO4 (aq) → 24. a) What volume(ml) of 0.115 M HCIO4 solution is required to neutralize 50.00 ml of 0.0875 M Ca(OH)2 ? b) A solution contains 3.2 g NaOH (MW = 40) in 20.0 ml of solution. What is the molarity of the solution? 25. A 44.0 g sample of an unknown metal at 99.0 °C was placed in a constant pressure calorimeter of negligible heat capacity containing 80.0 mL water at 24.0 °C. The final temperature of the system was found to be 28.4 °C. Calculate the Specific heat of the metal if density of water is 1.00 g/ml.

Answer 1

23. Ans :-

Balanced chemical equation is :

K₂CO₃ (aq) + H₂SO₄ (aq) --------------------> K₂SO₄ (aq) + H₂O (l) + CO₂ (g)

# Strong electrolytes are completely dissociated in aqueous solution. In this reaction strong electrolytes are:  K₂CO₃ , H₂SO₄ and K₂SO₄

# Weak electrolytes are partially dissociated in aqueous solution. In this reaction weak electrolytes are: H₂O (l) and CO₂ (g)

Therefore,

Complete balanced ionic equation is :

2 K+ (aq) + CO32- (aq) + 2 H+ (aq) + SO42- (aq) --------------------> 2 K+ (aq) + SO42- (aq) + H2O (l) + CO2 (g)

Here, K⁺ and SO₄^2- are spectators ions that is those ions which appear both side of complete ionic equation and cancel out when we write net ionic equation.

So,

Net ionic equation is :

CO32- (aq) + 2 H+ (aq) --------------------> H2O (l) + CO2 (g)