4. What is the pH of a 0.50 M solution of HC2H3O2?
HC2H3O2 is acetic acid, usually
written CH3COOH; it dissociates as follows:
CH3COOH ⇔ CH3OO- + H+, Ka =
1.8*10-5
0.50-x x x
If x moles of CH3COOH dissociate, x moles of
H+ and x moles of CH3COO- are
produced and the concentration of CH3COOH is reduced by x:
so Ka = x²/(0.50 - x)= 1.8*10-5
x²=1.8*10-5*(0.50 - x)
x will be small compared to 0.50, so Ka ≈ x²/0.50; x =
√[0.50*1.8*10^-5] = 0.003
[H+] = x = 0.003;
pH =-log([H+]) =-log(0.003)=2.52
thank you
To 1 L solution of 0.50 M HC2H3O2 and 0.50 M NaC2H3O2, 0.02 mol of solid NaOH was added. Calculate the pH of the resulting solution? Ka ( HC2H3O2) = 1.8 x 10-5. Use 3 sig.
1. Calculate the pH of 0.200 M HC2H3O2 (Ka of HC2H3O2 = 1.8 x 10-5) (2 pts) 2. Calculate the pH of a 0.10 M aqueous solution of sodium acetate, NAC2H3O2. (2 pts) asimtnsule A(da to 0H CHOH MOT o Um 007 0 3. A buffer solution contains 0.50 M acetic acid and 0.50 sodium acetate. Calculate the pH of this solution. (2 pts) ods odra J 0:0noiulo HOs l0 Jm 0.8 bbr po ard e ouce as toHenta erw...
1) What is the pH of a 0.085 M solution of acetic acid, HC2H3O2? At 25 degrees C, the Ka of acetic acid is 1.8 x 10^-5. 2) 17.4 mL of 4.0 M HCl are diluted with water to make 1.5 L of solution. What should be the pH of the final solution?
a solution that is 0.170 M in HC2H3O2 and 0.110 M in KC2H3O2 what is the pH? a solution that is 0.250 M in CH3NH2 and 0.135 M in CH3NH3Br what is the pH?
What is the pH of a buffer solution containing 0.13 M HC2H3O2 (acetic acid) and 0.11 M C2H3O2−?
Calculate the pH of a buffer solution that is 0.200 M in HC2H3O2 and 0.170 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Express your answer to two decimal places.
What is the pH of a solution containing 0.50 M ammonia and 0.50 M ammonium chloride? What will the pH be after 25mL of 0.20 M of hydrochloric acid has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? What will the pH be after 18mL of 0.25 M of lithium hydroxide has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? The ionization constant for ammonia is 1.8x10-5.
Find the pH of a.) a 0.725 M KC2H3O2 solution. The Ka of HC2H3O2 is 1.79 x 10-5 . b.) a 0.100 M NaCHO2 solution. The Ka of HCHO2 is 1.80 x 10-4 .
3. What is the pH of a solution that is 0.40 M NaBrO and 0.50 M HBrO (hypobromous acidy? (K, for HBrO 2.3 x 10 4. What is the pH of a solution in which 15 mL of 0.10 MNaOH is added to 25 mL of 0.10 M HCI?
Calculate the [H+] and the pH of a buffer solution that is 0.20 M in HC2H3O2 and contains sufficient sodium acetate to make the [C2H3O2-] equal to 0.20 M (Ka for HC2H3O2 = 1.8 x 10-5). (For scientific notation, enter your answer as follows: 1.0e-2 for 0.010)