Enter your answer in the provided box. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio [CH3COO−] / [CH3COOH].
Given, pH = 4.80
Now we know from the ka value tables the ka value for acetic acid = 1.8×10-5
So pKa = -log ka
pKa = -log (1.8×10-5)
=4.74
Now using handerson-hasselbalch equation,
pH= pKa+ log
pH - pKa = log
Putting values we get,
4.80 - 4.74 = log
0.06 =log
Or taking antilog , we get
= 100.06 = 1.14
So the ratio is,
= 1.14
Enter your answer in the provided box. The pH of a sodium acetate-acetic acid buffer is...
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You are making a pH 5.0 buffer with acetic acid (pKa = 4.75) and sodium acetate. You want the total concentration of acetate ([acetic acid] + [sodium acetate] ), to be 0.50 M. What concentrations of acetic acid and sodium acetate do you use to make your buffer? acetic acid sodium acetate
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0 mL of a CH3COOH (acetic acid)/ CH3COONa * 3H2O buffer. The target pH of the buffer is 5.25. The given concentration of [CH3COOH] is equal to 0.10 M. Ka = 1.80 x 10-5 for acetic acid. Use the Henderson-Hasselbalch equation to determine the ratio of [CH3COO-]/[CH3COOH] needed to make the buffer. pH = pKa + log([CH3COO-]/[CH3COOH]) Now calculate the concentration of acetate ion (CH3COO-...
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