Question

Given that the Ka of formic acid (HCHO2) is 1.80x10^-4, calculate the pH of a solution formed when 1.00 moles of sodium formate (NaCHO2) are dissolved in (and allowed to react with) 1.00L of distilled water. Question options: 5.13 7.00 8.87 1.80 12.20

Name: given that the ka of formic acid hcho2 is 180x10 4 calculate the ph of a solution formed when 100 moles of sodium formate nacho2 are dissolved in and allowed to react with 100l of distilled 00859
Uploaded: 2021-12-11T13:48:32-08:00
Duration: 1 min 27 s
Channel: Raghvendra Singh
Description: given that the ka of formic acid hcho2 is 180x10 4 calculate the ph of a solution formed when 100 moles of sodium formate nacho2 are dissolved in and allowed to react with 100l of distilled 00859

          Given that the Ka of formic acid (HCHO2) is 1.80x10^-4, calculate the pH of a solution formed when 1.00 moles of sodium formate (NaCHO2) are dissolved in (and allowed to react with) 1.00L of distilled water.
Question options:
5.13
7.00
8.87
1.80
12.20

Added by Justin M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Raghvendra Singh

12/11/2021

Step 1

Step 1: Write the balanced chemical equation for the reaction between sodium formate and water: NaCHO2 + H2O -> HCHO2 + NaOH Show more…

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Given that the Ka of formic acid (HCHO2) is 1.80x10^-4, calculate the pH of a solution formed when 1.00 moles of sodium formate (NaCHO2) are dissolved in (and allowed to react with) 1.00L of distilled water. Question options: 5.13 7.00 8.87 1.80 12.20