Calculate the ph of a buffer that is 0.225 m hc2h3o2 and 0.162 m kc2h3o2. the ka for hc2h3o2 is 1.8 Ã 10-5. 4.60 9.26 4.74 4.89 9.11 - 9081563

A buffer solution contains 0.32 mol of acetic acid (HC2H3O2) and 0.41 mol of sodium acetate (NaC2H3O2) in 7.40 L. The Ka of acetic acid (HC2H3O2) is Ka = 1.8e-05. (a) what is the pH of this buffer? (b) what us the pH of the buffer after the addition of 0.12 mol of NaOH? Nov 10, 2012 · A buffer solution acetic acid (HC2H3O2) at a concentration of 0.225 M and sodium acetate ( NaC2H3O2) at a concentration of 0.164 M. The value of Ka for acetic acid is 1.75 X 10^-5. calculate the pH of this solution using the Hendersen- Hasselbalch equation. Hey guys, I was wondering if anybody could tell me if these are right? Write two equations showing how the HC2H3O2/NaC2H3O2 buffer uses up added H+ ions and OH- ions. 1. HC2H3O2 + H3O+ ---> H2C2H3O2 + H2O 2. NaC2H3O2 + OH- ---> C2H3O2- + H2O Write two equations showing how the NH3/NH4Cl buffer uses up added H+ ions and OH- ions. 1. A solution containing which one of the following pairs of substances will be a buffer solution? in a solution that contains 0.025 M of CO3^2-. 0.820 M HC2H3O2 The pKa of acetic acid, HC2H3O2, is 4.76. A buffer solution was made using an unspecified amount of acetic acid and 0.30 moles of NaC2H3O2 in enough water to make 2.00 liters of solution. Its pH was measured as 4.40. weak acid (HC2H3O2) in the buffer. NaOH(aq) + HC2H3O2(aq) H2O(l) + NaC2H3O2(aq) • If the amount of NaOH added is less than the amount of acetic acid present, the pH change is small. • If a strong acid is added, it is neutralized by the conjugate base (NaC2H3O2) in the buffer. HCl(aq) + NaC2H3O2 HC2H3O2(aq) + NaCl(aq)

## If a solution initially contains 0.260 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 ∘C? Express your answer in moles per liter to two significant figures.

Predict whether a precipitate of MgF2 will form when 100.0 milliliters of a 3.00 10-3-molar Mg(NO3)2 solution is mixed with 200.0 milliliters of a 2.00 l0-3-molar NaF solution at 18ºC. Calculations to support your prediction must be shown. At 27ºC the concentration of Mg2+ in a saturated solution of MgF2 is 1.17 10-3 molar.

### Solution: 1) This is a buffer solution, with a weak base (the ammonia) and the salt of the weak base (the ammonium chloride) in solution at the same time. We must use the Henderson-Hasselbalch equation to solve this problem. pH = pK a + log [base / acid] 2) We know the two concentrations: pH = pK a + log [0.25 / 0.35]

Notes - Buffers & Titrations.pdf page 1 of 11. 1 ap chemistry chapter 17 applications of aqueous equilibria reactions and equilibria involving acids, bases, and salts common ions