Topic: pH of OH in HCO3- (Read 8299 times)

soupastupid · « **on:** October 14, 2008, 08:26:52 PM »

Determine the [OH^-] of a solution that is 0.230 M in HCO_3^-

Then Determine pH of solution.

soupastupid · « **Reply #1 on:** October 14, 2008, 09:25:51 PM »

is [OH-]

2.25*10^-6

and is the pH 8.40

Borek · « **Reply #2 on:** October 15, 2008, 05:29:16 AM »

Question - as worded - has no solution. pH will depend on the amount of CO₃^2- and H₂CO₃ present.

I suppose what you mean is what is pH of solution that was initially 0.230M in HCO₃^- with no other substances (but a simple counterion) present.

If so, your answer is close to the reality.

AWK · « **Reply #3 on:** October 15, 2008, 07:07:24 AM »

Aproximate formula for NaHCO₃ is
[H3O+] = SQRT(K_a1K_a2) which gives pH close to 8.1 taking into account also the ionic strength.

soupastupid · « **Reply #4 on:** October 15, 2008, 04:59:36 PM »

its not working

soupastupid · « **Reply #5 on:** October 15, 2008, 05:29:36 PM »

does this look right?

Borek · « **Reply #6 on:** October 15, 2008, 06:33:00 PM »

You have ignored HCO₃^- <-> H⁺ + CO₃^2-.

http://www.chembuddy.com/?left=pH-calculation&right=pH-amphiprotic-salt

Topic: pH of OH in HCO3- (Read 8299 times)

soupastupid

pH of OH in HCO3-

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AWK

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