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13 Dec 2019

Calculate pH (Henderson–)

A buffer solution is 0.364 M in HNO2 and 0.262 M in KNO2. If Ka for HNO2 is 4.5×10-4, what is the pH of this buffer solution?

A buffer solution is 0.483M in H3PO4 and 0.226 M in NaH2PO4. If Ka forH3PO4 is 7.5×10-3, what is the pH of this buffer solution?

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Related questions

What is the [H3O+] and the pH of a buffer that consits of 0.49 MHNO2 and 0.66 M KNO2?

(Ka of HNO2 = 7.1 x 10^-4)

What is the [H3O+] and the pH of a buffer that consits of 0.49 MHNO2 and 0.66 M KNO2?

(Ka of HNO2 = 7.1 x 10^-4)

A.)Calculate the pH of the buffer that results from mixing 51.0 mL of a 0.488 M solution of HCHO2 and 16.0 mL of a 0.571 M solution of NaCHO2. The Kavalue for HCHO2 is 1.8×10−4.

B.)Consider a buffer solution that is 0.50

M in NH3and 0.20 M in NH4Cl. For ammonia,=pKb 4.75 Calculate the pH of 1.0 L of the solution, upon addition of 49.00 mL of 1.0

C.)A 36.0 mL sample of 0.162 M HNO2 is titrated with 0.226 M KOH. (Ka for HNO2 is 4.57×10−4.)Determine the pH at the equivalence point for the titration of HNO2 and KOH

D.)A 1.0-

L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Calculate the

pH of the solution upon addition of 19.1 mL of 1.00 MHCl
to the original buffer.MHClpKb=4.75

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