A buffer solution contains 0.327 M acetic acid and 0.402 M sodium acetate. If 0.0258 moles of hydrobromic acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrobromic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining

e and le akeCovakiAcivity dolorntor asinnment-take [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution contains 0.305 M NH,CI and 0.338 M NH3 (ammonia). Determine the pH change when 0.089 mol KOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change = Submit Answer Retry Entire Group 1 more group attempt remaining erevs Next ENG 令 D US Home End Areert & 7 8

bha Please don't provide handwritting solution

please answer both for a vote uofront. thanks (Please type answer no write by hend)

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Part A Review Constants | Periodic Table Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH, COO). Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base: H++ CH3COO→CH3COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid: OH +…

please don't provide handwritten solution..

A buffer solution is 0.418 M in HCN and 0.307 M in NaCN. If Ka for HCN is 4.0 × 10-¹0, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 2 more group attempts remaining

Use the References to access important values if needed for this question. A buffer solution is 0.386 M in KHSO3 and 0.338 M in K2 SO3. If K, for HSO3- is 6.4 x 10-8, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining

Solve correctly please , need both subparts to be solve.