A 26.50 mL solution of Fe2+ required 17.50 mL of 0.175 M KMNO, to reach the end point. 5 Fe2 + (aq) + MnO,(aq) + 8 H† 5 Fe3 +(aq) + Mn² +(aq) + 4 H,O(1) Calculate the concentration of the Fe2 + solution. [Fe? +] = M
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- solve the following parts a. Would the addition of K2SO4 to a saturated solution of CaSO4 cause the solubility to increase or decrease? Explain your answer in words not with a calculation. b. Balance the following redox reaction under basic conditions. Cr(OH)3(s) + TiO2(s)→Ti2+(aq) + CrO42-(aq)Balance in acid medium: iodate ion + sulfite ion : then {HNO3} : iodine + sulfate ion 10 ml of 6N HNO3 are mixed with 15 ml of 10N sodium sulfite. How many milliliters of 1.4 M sodium iodate are needed for the reaction to take place?The following solubility equilibrium has K = 2.8 x 10–3 at 25oC. AgCl(s) + 2NH3(aq) ⇌ Ag(NH3)2+(aq) + Cl–(aq) How many grams of AgCl (molar mass = 143.35 g/mol) will dissolve in 5.0 x 102 mL of 2.0 M NH3 solution at 25oC? (A) 0.76 g (B) 6.9 g Is the correct answer (A) or (B)?
- A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0948 M HBr. It required 64.6 mL of the acid solution for neutralization.(a) What was the molarity of the Ca(OH)2 solution? M(b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mLMg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.200 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH.(Eqn. 1) 1 OCl− + 3 I− + 2 H+ → 1 I3− + 1 Cl− + 1 H2O (Eqn. 2) 2 S2O32− + 1 I3− + 0 H+ → 3 I− + 1 S4O62− + 0 H2O Multiply Equation 2 by the molar ratio of 1/1 and add to Equation 1 to obtain the overall balanced net ionic equation for the titration of the diluted bleach sample. 1) What is the molar ratio of OCl− to S2O32− in the overall net ionic equation?
- The solubility of Mn(OH)2 in water is 0.0002 g/100 mL. What is the solubility in gramformula weights per liter in a solution which is 0.01F with respect to the hydroxide ions?Given 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.A group of students determined the concentration of iodate ion in a solution sample through titration, based on the above equation. If 28.1 mL 0.200 M S2O32- solution was used to reach the endpoint, calculate the millimoles of iodate ion in the sample. Show your result in four decimal place
- A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.Calculate the concentration of cobalt(III) ions in a solution formed by mixing 200 mL of 0.200 M Co(NO3)3 with 250 mL of 5.00 M NH3 solution given Kf of [Co(NH3)6]3+ is 4.5×1033. [Co3+] = ___M4 A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0771 M HBr. It required 86.7 mL of the acid solution for neutralization. (a) What was the molarity of the Ca(OH)2 solution? M (b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution? g/100mL