Solution Found!
A chemist dissolves 0.135 mole of CO2(g) in 2.50 L of
Chapter 7, Problem 7.166(choose chapter or problem)
QUESTION:
A chemist dissolves 0.135 mole of CO2(g) in 2.50 L of 0.105 M Na2CO3. Calculate the pH of the resulting solution
Questions & Answers
QUESTION:
A chemist dissolves 0.135 mole of CO2(g) in 2.50 L of 0.105 M Na2CO3. Calculate the pH of the resulting solution
ANSWER:
.
The reaction is as follows:
CO2(g) + 2Na2CO3 (aq) ? 2NaHCO3 (aq) + Na2CO3 (aq)
The amount of Na2CO3 that is needed to react with the CO2 is equal to the molar ratio of Na2CO3 to CO2 in the given reaction, which is written as follows:
Moles of Na2CO3 = (
The reaction is as follows:
CO2(g) + 2Na2CO3 (aq) ? 2NaHCO3 (aq) + Na2CO3 (aq)
The amount of Na2CO3 that is needed to react with the CO2 is equal to the molar ratio of Na2CO3 to CO2 in the given reaction, which is written as follows:
Moles of Na2CO3 = (