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- Consider this reaction H2SO4(aq) +2KOH(aq) ---> H2SO4(aq) ---->K2SO4(aq) +2H2O(l) Determine the volume of 0.205 M KOH solution require to neutralize each sampe of sulfuric acid. a. 35mL of 0.205 M H2SO4 b. 205mL of 0.135 M H2SO4 C. 80 ml of 0.100 M H2SO4Zn(s) + 2 Ag+ (aq) ® Zn2+(aq) + 2 Ag(s) What would happen to the value of Ecell if the concentration of Ag+ and Zn+2 are both cut in half. It would increase It would decrease It would not change Not enough information to tella. Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq) b. If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint?
- What should be the coefficient of BiO3- in order to balance the reaction: Mn2+ + BiO3- ---H+----> MnO4- + Bi3+Which of the following reactions will occur spontaneously as written? Explain your answer.a. 3Fe2+(aq) + Cr3+(aq) ==> Cr(s) + 3 Fe3+(aq)b. Sn2+(aq) + Fe2+(aq) ==> Sn4+(aq) + Fe3+(aq)c. Sn2+(aq) + Fe(s) ==> Sn4+(aq) + Fe2+(aq)d. 2Cr3+(aq) + 3 Sn2+(aq)==> 3Sn4+(aq) + 2Cr(s)Consider the neutralization reaction. 2HNO3(aq) + Ba(OH)2(aq) -->2H2O(I) + Ba(NO3)2(aq) A 0.110 L sample of an unknown HNO3 solution required 41.7mL of 0.100 M Ba(OH)2 for complete neutralization. What is the concentration oh the HNO3 solution? concentration:____M
- The following reactions (note that the arrows are pointingonly one direction) can be used to prepare an activity seriesfor the halogens:Br2(aq) + 2 NaI(aq)----->2 NaBr(aq) + I2(aq)Cl2(aq) + 2 NaBr(aq)----->2 NaCl(aq) + Br2(aq)(a) Which elemental halogen would you predict is the moststable, upon mixing with other halides? (b) Predict whethera reaction will occur when elemental chlorine and potassiumiodide are mixed. (c) Predict whether a reaction will occurwhen elemental bromine and lithium chloride are mixed.A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The resulting solution is titrated with a NaOH solution of unknown concentration. If 21.50 mL of the base solution is needed to reach the end-point, what is the molar concentration of NaOH solution? The reaction occurs as follows: NaOH(aq) + KHC8H4O4(aq) --> NaKC8H4O4(aq) + H2O(l) (A) 0.2457 M (B) 0.1254 M (C) 0.05390 M (D) 0.03823 MGiven the equation Ag(aq)+ + 2NH3(aq) ----> [Ag(NH3)2]+(aq), determine the concentration of NH3(aq) that is required to dissolved 261mg of AgCl in 100 ml of solution. The Ksp of AgCl is 1.77 x 10-10 Kf = 2 x 107.
- The titration of 25.00 mL of an unknown concentration of H2SO4 solution requires 32.28 mL of 0.420 M LiOH solution. What is the concentration of the H2SO4 solution in units of molarity (M)? H2SO4(aq)+2LiOH(aq)--->Li2SO4(aq)+2H2O(l)Calculate the value of Keq. How well do these values compare to each other? Fe3 = 0.002 M , SCN = 0.002 M Keq= [FeSCN^2]/ [Fe^3][SCN^-]Suppose, in an experiment to determine the amount of sodium hypochlorite in bleach, you titrated a 22.84 mL22.84 mL sample of 0.0100 M KIO30.0100 M KIO3 with a solution of Na2S2O3Na2S2O3 of unknown concentration. The endpoint was observed to occur at 12.07 mL12.07 mL . How many moles of KIO3KIO3 were titrated?
