1. What is the pH of a water that contains 120 mg/L of bicarbonate and 15 mg/L of carbonateions?Hint: remember to use the equilibriums as follows:(H*][HCO;"] - KAL - 4.47 x 107 mol/L[H, CO,][H*][CO,²][HCO,]KA2 = 4.68 x 10" mol/L%3D

Given: Concentration of bicarbonate i.e. HCO3- = 120 mg/L. And concentration of carbonate i.e. CO32-…

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1. What is the pH of a water that contains 120 mg/L of bicarbonate and 15 mg/L of carbonate ions?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 38QAP: To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of...

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Question

1. What is the pH of a water that contains 120 mg/L of bicarbonate and 15 mg/L of carbonate
ions?
Hint: remember to use the equilibriums as follows:
(H*][HCO;"] - KAL - 4.47 x 107 mol/L
[H, CO,]
[H*][CO,²]
[HCO,]
KA2 = 4.68 x 10" mol/L
%3D

Expert Solution

Step 1

Given: Concentration of bicarbonate i.e. HCO₃^- = 120 mg/L.

And concentration of carbonate i.e. CO₃^2- = 15 mg/L.

Molar mass of HCO₃^- is 61 g/mol and that of CO₃^2- is 60 g/mol.

$S i n c e m o l a r c o n c e n t r a t i o n = \frac{C o n c e n t r a t i o n i n m g / L}{M o l a r m a s s \times 1000} H e n c e m o l a r c o n c e n t r a t i o n o f H C {O_{3}}^{-} = \frac{120}{1000 \times 61} = 0.0019672 M a p p r o x . A n d m o l a r c o n c e n t r a t i o n o f C {O_{3}}^{2 -} = \frac{15}{1000 \times 60} = 0.000250 M .$

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