Select the charge balance equation for an aqueous solution of MnCl, that ionizes to Mn2+, Cl",...
Select the mass balance equation for the same solution. O2([Mn2+1+ [MnCit]+[MnOH]) = [MnCit] + [C1"] O [Mn2+1+ [MnCit] + [MnO4+1 = [MnCit]+2 [C1"] 2[Mn2+] = [C1"] O 2 [Mn2+] + [MnCit] + [MnOH'] = [Mncit]+[C1"] O [Mn2+] = 2 [C1"] O [Mn2+1 + [MnCit] + [MnOH"] = 2 ([MnCit]+[C1-])
Write a charge balance for an aqueous solution of H2SO4 in water if the H2SO4 ionizes to HSO4- and SO42-
Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution. Cl−(aq)+MnO4−(aq)→Cl2(g)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
(a) Consider the following chemical reaction in acidic aqueous solution: ?MnO4- + ?H2O2+cH+ → ?Mn2++?O2+?H2O Write down (but do not solve) equations that we could use to balance this reaction by Gaussian elimination. Specify what is being “conserved” in front of each equation. (b) Suppose we let ? = 1. Could the reaction then be balanced with exactly one set of numbers ?, ?, ?, ?, ?? (Y/N)
1.00 m aqueous solution of trichloroacetic acid (CCl3COOH) ionizes according to the following equation: CCl3COOH (aq) ⇌ H+ (aq) + CCl3CO2- (aq) Determine the pH of the solution if it freezes at -2.53oC. (KF of water = 1.86oC/m) (Assume that the molality and the molarity of the solution are the same.)
Problem 1: Balance the following reaction in (a) acidic solution and (b) basic solution MnO2 (s) + H Asos (aq) → Mn2+ (aq) + HASO (aq) (a) Acidic solution 1. Split the reaction into two half-reactions. Mn q + ac Mnat HAs Oy > Hj As Oy + ae" 2. Consider the following half reaction: MnO2 (s) → Mn2+ (aq) Balance everything but oxygen and hydrogen atoms. MnOade > Moi 3. Take your answer to (2) and balance the oxygen...
ca 2. What is the charge balance for an aqueous solution of arsenic acid, H3AsO4, in which the acid can dissociate to H2AsO4 , HASO4+-, and AsO4”. a) [H+] = [OH-] + [H2AsO4] + 2[HASO42-] + 3[AsO43-] (b) [H+] = [OH-] + [H2AsO4] + [HASO42-] + [AsO43-] c) [H+] = 2[OH-] + 2[H2AsO4] + 2[HASO42-] + 2[AsO43-] d) [H3AsO4) = 2[H2As04] + 2[HAsO42-] + 2[AsO4?]
balance these equations
MnCl2 + KCI+ Cl+ HO (CI is chlorine in this equation) KMnOs+ HCI Ca(CIO)2+ HCI-CaCla+ H2O+ Clh (Cl is chlorine in this equation) O2 PbO+ CO:+ H:O Pb(CaHs) P.OtO+ H.OHPO CO2+ HO+ NH 4 increal C H12O$N;+ O es, the l thematical
5. Given the following incomplete redox reaction, balance this equation in ACID solution with the set of smallest whole number coefficients: MnO2 + Cl(aq) ---> Mn²+(aq) + Cl2(g) To balance the above redox equation requires: a) 4 OH on the left and 4 H+ on the right. b) 4 H+ on the left and 2 H20 on the right. c) 8 H on the left and 4 H20 on the right. d) 4 H20 on the left and 2 H+...
Part A the value of Ky at that temperature? Water ionizes by the equation H2O(l) = 1+ (aq) + OH-(aq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between (H+) and (OH): Ky = [H+][OH-] Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. At a certain temperature, the pH of a neutral solution is 7.65. What Express your answer numerically using...