Question

In experiment 1 you prepared a solution of sodium carbonate. This means you dissolved solid Na2CO3 in water. Since this ionic compound dissolved in water, you now have only its ions swimming around in the solution. What are the aqueous ions in your solution of sodium carbonate? TTT Arial # 3 (12 # TEE Path: p Words:04 QUESTION 2 In experiment 2, you used a solution of HCI. HCl is a strong acid, which means it is 100% ionized in solution. Write the aqueous ions that exist in the solution of HCI. TTT Arial 4 3 (124 TEE Path: p Words:0 QUESTION 3 In experiment 2, you combined the solutions of sodium carbonate (a base) and hydrochloric acid (an acid). Write the ions that exist in these two solutions as your reactants in a neutralization reaction. Exchange ion partners to figure out what the products of the reaction are (H2CO3 is one of the products.) Write a balanced chemical equation for this reaction. TTT Arial # 3 (12 T. Path:p Words:0 QUESTION 4 Carbonic acid, H2CO3, is unstable in solution. The H2CO3 will decompose to form carbon dioxide and water. Write a balanced chemical reaction for this decomposition reaction.

Answer 1

Question 1 : Ionic Na, coz dissolved in water as below - Na CO₂ (s) + H20le) 2 Nat (aq) + cor (ar) Thus the aqueous ions in the soluti- on of sodium carbonate are - Nat (ar) and coz (ar) guestion 2 : Her is stroong acid and 100% ioni- zable in solution. Hel (as) H+ (aq) + ct (ar). Aqueous ions that exist in the solution of Hel are - H + (ar) and it (ar) question 3 : The balanced equation for the neutralisation can be given as - reaction.

2 Na (ar) & cor (ar) + 2H+ (aq) +201 (ar) H₂ CO₂ (ar) +2Nach (ar) Question 4 : Hq CO₂ will decompose to form carbon dioxide and water The balanced chemical equation can be given as - Hq CO₂ (ar) H20 (1) + coz (9)