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A 1.0-L buffer solution contains 0.100 mol? HC2H3O2 and 0.100 mol? NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10?5. You may want to reference (Pages 781 - 791) Section 17.2 while completing this problem. Part A Calculate the pH of the solution, upon addition of 0.010 mol of NaOH to the original buffer. Express y

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17 Dec 2019

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Related questions

A 1.0L buffer solution contains 0.100 mol of HC2H3O2 and 0.100 mol of NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.

Calculate the pH of the solution upon the addition of 0.015 mol of NaOH to the original buffer.

Part A

Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.​

Calculate the pH of 1.0 L of the original buffer, upon addition of 0.190 mol of solid NaOH.

Part B

A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.​

Calculate the pH of the solution, upon addition of 0.030 mol of NaOH to the original buffer.

(I will leave a good rating, thank you)

A 1.0 L buffer solution contains 0.187 M HC2H3O2 and 0.187 M NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa=−log(1.8×10−5)=4.74. Part A Calculate the new pH after adding 0.019 mol of solid NaOH to the buffer.

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