I caution you that m means molality. M means molarity. I assume you meant M.
Use the Henderson-Hasselbalch equation.
a = acid; b = base.
pH = pKa + log(b/a)
4.5 = 4.75 + log b/a
solve for b/a and I get approximately 0.6 (you should do it more accurately).
You have two unknowns and you need a second equation. That one is
a + b = 0.08
Solve the two equations simultaneously. I get a = about 0.05M and b = about 0.03M.
Now you have 500 mL of the buffer so you have how many millimoles of a and b?
500 x 0.05 = about 25 mmoles acid.
500 x 0.03 = about 15 mmoles base.
...........Ac^- + H^+ ==> HAc
add............10(100 x 0.1 = 10 mmol)
Again, these are approximate; you need to go through the calculations more accurately.
Then plug these equilibrium concns into the HH equation and solve for pH.
I arrived at 3.84.
. Use the Henderson-Hasselbach equation: pH = pKa + log [A-]/[AH], where A- is the conjugate base and AH is the weak acid. Calculate the pH of an acetate buffer in which the acetate concentration [CH3COO-] is 3.5 times greater
How to start these problems out: Please help thank you Use the Henderson-Hasselbach equation: pH = pKa + log [A-]/[AH], where A- is the conjugate base and AH is the weak acid. Calculate the pH of an acetate buffer in which the
What is the pH of 0.1 M formic acid solution? Ka=1.7„e10-4? What is the pH value of buffer prepared by adding 60 ml of 0.1 M CH3COOH to 40 ml of a solution of 0.1 M CH3COONa? What is the pH value of an acetate buffer (pK=4.76)
A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer? A. .01 mol B. .05 mol C.
1). Calculate the initial and final pH when 5.0, 10.0, and 100mL of 0.100M HCL is added to (a) 100mL of water (b) 100mL of a buffer which is 1.50M acetic acid and 1.20M sodium acetate 2). Develop a recipe for making this buffer
a solution is made by combining 10.0 ml of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. a)calculate the pH of the solution. b) how many grams and milliliters of 14.6 M potassium