**Determining the Concentration of a Copper(I) Solution**The concentration of a Cu\(^+\) solution is determined by titrating it with a 0.1395 M solution of permanganate. The balanced net ionic equation for the reaction is:\[ \text{MnO}_4^-(\text{aq}) + 5 \, \text{Cu}^+(\text{aq}) + 8 \, \text{H}_3\text{O}^+(\text{aq}) \rightarrow \text{Mn}^{2+}(\text{aq}) + 5 \, \text{Cu}^{2+}(\text{aq}) + 12 \, \text{H}_2\text{O(l)} \]**Experiment Details:**In one experiment, 21.54 mL of the 0.1395 M MnO\(_4^-\) solution is required to react completely with 40.00 mL of the Cu\(^+\) solution. Calculate the concentration of the Cu\(^+\) solution. \[\text{Concentration of Cu}^+\text{ solution: } \boxed{\, \, \, \, \, \, \, \, \, \,}\text{ M} \]

This problem can be solved by using the molarity equation :…

The concentration of a Cu* solution is determined by titrating it with a 0.1395 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. MnO, (aq) + 5 Cu*(aq)+8 H3O*(aq)- Mn2*(aq) + 5 Cu²*(aq)+12 H,0(1) In one experiment, 21.54 mL of the 0.1395 M MnO, solution is required to react completely with 40.00 mL of the Cut solution. Calculate the concentration of the Cut solution. M

The concentration of a Cu* solution is determined by titrating it with a 0.1395 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. MnO, (aq) + 5 Cu(aq)+8 H3O(aq)- Mn2(aq) + 5 Cu²(aq)+12 H,0(1) In one experiment, 21.54 mL of the 0.1395 M MnO, solution is required to react completely with 40.00 mL of the Cut solution. Calculate the concentration of the Cut solution. M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Given the following unbalanced equation, select the correct net ionic equation. CaCO3(s) + HCI(aq) CaCl2(aq) + H20(1) + CO2(g) --> (A) Ca2*(aq) + 2CI^(aq) CaCl2(aq) --> (B) CO32-(aq) + 2H*(aq) --> H20(1) + CO2(g) (C) CaCO3(s) + 2H*(aq) + 2CI¯(aq) CaCl2(aq) + H20(1) + CO2(g) --> (D) CaCO3(s) + 2H*(aq) --> Ca2*(aq) + H20(1) + CO2(g)
A 14.0 mL sample of vinegar, which is an aqueous solution of acetic. acid, CH₂COOH, requires 22.5 mL of a 0.700 M solution of NaOH to reach the endpoint in a titration: CH₂COOH(aq) + NaOH(aq) → NaCH,COO(aq) + H₂O(1) Part A What is the molarity of the acetic acid solution? Express the concentration to three significant figures and include the appropriate unit Value Submit Units Request Answer ONE ?
The concentration of H₂AsO3 in a solution is determined by titrating it with a 0.1722 M Ce solution. The balanced net ionic equation for the reaction is: 2Ce+ (aq) + H₂AsO3(aq) + 5H₂0 (1) 2Ce³+ (aq) + H₂AsO4(aq) + 2H30+ (aq) In one experiment, 21.40 ml of the 0.1722-M Ce4+ solution is required to react completely with 40.00 mL of the H₂AsO, solution. Calculate the concentration of the H₂AsO solution. Submit Show Approach Show Tutor Steps
Write net ionic equations for the following reactions:
The amount of chloride anion in a solution can be determined via titration with AgNO3(aq), according to the following balanced chemical equation: Cl–(aq) + AgNO3(aq) → AgCl(s) + NO3–(aq) What is the molarity of NaCl in a solution if titration of 15.00 mL of the solution with 0.2488 M AgNO3 requires 19.13 mL of the AgNO3 solution to reach the endpoint.
The concentration of hydrogen peroxide in a solution is determined by titrating it with a 0.1217 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnO4 (aq) + 5H₂O₂ (aq) + 6H3O+ (aq) → 2Mn²+ (aq) +50₂ (1) + 14H₂O(1) In one experiment, 19.09 mL of the 0.1217 M permanganate solution is required to react completely with 40.00 mL of the hydrogen peroxide solution. Calculate the concentration of the hydrogen peroxide solution. Concentration = M
The iron content of iron ore can be determined by titration with K₂Cr₂O₇ according to the equation 14H⁺(aq) + Cr₂O₇²⁻(aq) + 6Fe²⁺(aq) → 6Fe³⁺(aq) + 2Cr³⁺(aq) + 7H₂O(l) Diphenyl amine is used as an indicator as it changes color from green to purple when the endpoint is reached. A sample of iron ore with a mass of 3.255 g was dissolved with HCl and then treated with a reducing agent to convert any Fe³⁺ in the ore to Fe²⁺. Titration with 0.0645 M K₂Cr₂O₇ solution required 45.65 mL of the solution to reach the endpoint. The molar mass of Fe is 55.85 g/mol. Calculate the mass percent iron in the ore.
Complete the following reaction and balance it. Fe(OH)3(aq) + HCl(aq) → a) FeCl3(aq)+ 3 H2O(l) b) FeCl(aq) + H2O(l) c) Fe(aq) + HOCl(aq) d) FeCl(aq) + 3 OH–(aq) e) H2O(l) + FeCl2(aq)
Classify the reactions represented by these equations as either single or double placement.
14 In the equation 2Na*(aq) + C0,2-(aq) + Sr2+(aq) + 2Cl-(aq) SPCO,(s) + 2Na*(aq) + 2Cl-(aq) (a) Identify the spectator ions. (b) Write the balanced net ionic equation.
The concentration of a Fe2+ solution is determined by titrating it with a 0.1934 M solution of dichromate. The balanced net ionic equation for the reaction is shown below. Cr2O72-(aq) + 6 Fe2+(aq)+14 H3O+(aq)2 Cr3+(aq) + 6 Fe3+(aq)+21 H2O(l) In one experiment, 17.15 mL of the 0.1934 M Cr2O72- solution is required to react completely with 25.00 mL of the Fe2+ solution. Calculate the concentration of the Fe2+ solution.
A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s) How many moles of Ag+ (aq) ions are used to reach the end point? How many moles of Cℓ- (aq) have reacted in the titration? How many grams of chloride are present in the sample? What is the mass percent of chloride in the sample?