What is the pH of a solution obtained by mixing equal amounts of 0.010 M solutio

Question

What is the pH of a solution obtained by mixing equal amounts of 0.010 M solutions of nitrous acid and potassium hydroxide? pH=7.0 because this is a neutralization reaction pH 7.0 because there will be more hydronium ion than hydroxide ion in the solution For which of the salts listed below can you calculate the pH of the solution without needing to know the concentration of the solution? NH_4Cl NaCN MgHPO_4 Lil Both c and d What is the molarity of KCH_3COO solution if its pH is 8.65? 4.5 times 10^-6 M 5.0 times 10^-8 M 2.4 times 10^-5 M 3.6 times 10^-2 M 2.8 times 10^-13 M For questions 28-29 consider 650 mL of 0.880 M ammonium buffer at pH 9.25. The buffer contains _____________ moles ammonium ion and __________ moles ammonia? 0.880 0.440 0.572 0.572 0.440 0.440 0.572 0.286 0.286 0.286 What is the buffer capacity of this buffer towards the addition of 0.55 M HC1? 129 mL 234 mL 425 mL 520 mL 650 mL The titration of _____________ with ________________ will have an equivalence point at pH

Explanation / Answer

answer is a

balance equation

HNO2(aq) + KOH(aq) ===> KNO2(aq) + H2O

it is a neutralising reaction = Ph 7

reason

all the H+ ions produced by HNO2 is neutralised by OH- of KOH resulting water molecules so Ph is 7

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.