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A buffer solution is prepared by adding 25 mL of 0.050 M sulfuric acid solution to 50 mL of 0.10 M ammonia solution. What is the pH of the buffer?

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Related questions

Calculate the pH of the following buffer solutions: (anwers given in bold)

1) A solution obtained by adding 30 mL of 0.20 M HOAc to 25 mL of 0.10 M NaOH. R = 4.61

2) A solution that is 0.050 M in formic acid and 0.10 M in sodium form. R = 4.0

3) A buffer solution of acetic acid-sodium acetate of pH 5.00 (initial) whose concentration in NaOAc is 0.100 M, after the addition of 10 mL of 0.1 M NaOH to 100 mL of the buffer. R = 5.12

A 500.0 mL buffer solution is 0.10 M in benzoic acid and 0.10 M in sodium benzoate. What is the pH of the buffer before and after addition of 200 mL of 0.050 M NaOH?

Soduim acetate molecular weight is 136.08

the mass of 10 mmol of this sodium acetate is 1.3608g

Ammonium chloride molecular weight is 53.49

The mass of 10 mmol of this ammonium chloride is0.5349 g

a)

0.10 M Acetate Buffer Solution:

pH of 0.10 M acetic acid solution is 2.53(experimantally)

pH of 0.10 M acetate buffer solution is 3.80 (expermantally)


1) 1.1 ml of 1.0 M HCl , what the calculated pH foradding this strong acid (HCl) ? the measured value was 3.61.


2) 1.0 ml of 1.0 M NaOH, what the calculated pH foradding this strong base(NaOH) ? the measured value was 3.98.


b)

0.10 M Ammonia buffer solution:

pH of 0.10 M ammonia solution is 10.83 (experimantally)

pH of 0.10 M ammonia buffer solution is 9,87 (experimantally)


1) 1.1 ml of 1.0 M HCl , what thecalculated pH for adding this strong acid (HCl)? the measured value was9.73.


2) 1.1ml of 1.0 M HCl , what the calculated pH for adding this strongbase (NaOH) ?the measured value was 9.98.


I have no clue how this work. itsays this can be solved by usingHenderson-Hasselbalch equation. I need help please

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