What is the molarity of ZnCl 2 that forms when 25.0 g of zinc completely reacts with CuCl 2 according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl 2 (aq) → ZnCl 2 (aq) + Cu(s)

Hello everyone. Today we have a phone problem. What is the molarity of zinc chloride that forms when 25 g of zinc completely reacts with copper chloride according to the following reaction, assume a final volume of 275 mL. So first, we want to start with our given which was 25 g of zinc. Let me want to do a couple of conversions. The first is we want to do a molar mass conversion, which if we look at the periodic table, we can state that one mole of zinc is equal or equivalent to 65.39 g of zinc. From there, we want to perform a multiple ratio to get from moles of zinc to moles of zinc chloride. And so if we look at our equation, we see that we used one mole of zinc to create or to produce one mole of zinc chloride. We then like in our unit. So far, we can cancel out grams of zinc and moles of zinc. So recall that molar mass is the grams over moles or moles over grams. So what we can do is we can multiply one final our molarity is what we need to solve for is going to be moles over liters. So we can multiply by our 275. But we can say that we have our 1/2 75 mL can be multiplied. Brother Rachel, that 1 mL is equal to 10 to the negative third liters. When those units cancel, we are left with 1.39 molar molars of zinc chloride. And with that, we're gonna conclude our answer c overall, I hope it helped. And until next time.

Ch.5 - Introduction to Solutions and Aqueous Solutions

All textbooks

Tro 5th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 36

Previous problem

Next problem

Chapter 5, Problem 36

What is the molarity of ZnCl₂ that forms when 25.0 g of zinc completely reacts with CuCl₂ according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl₂(aq) → ZnCl₂(aq) + Cu(s)

Verified step by step guidance

Determine the molar mass of zinc (Zn) using the periodic table.

Calculate the moles of zinc (Zn) using the formula: \( \text{moles of Zn} = \frac{\text{mass of Zn}}{\text{molar mass of Zn}} \).

Use the stoichiometry of the balanced chemical equation to find the moles of ZnCl_2 produced. Note that the reaction is a 1:1 ratio between Zn and ZnCl_2.

Calculate the molarity of ZnCl_2 using the formula: \( \text{Molarity} = \frac{\text{moles of ZnCl}_2}{\text{volume in liters}} \).

Convert the final volume from milliliters to liters by dividing by 1000.

Verified Solution

Video duration:

0m:0s

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (mol/L). To calculate molarity, one must know the amount of solute in grams, convert it to moles using its molar mass, and then divide by the volume of the solution in liters.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows us to determine the amount of product formed or reactant consumed by using mole ratios derived from the coefficients in the balanced equation. In this case, it helps to relate the amount of zinc used to the amount of ZnCl2 produced.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. For this problem, knowing the molar mass of zinc (Zn) and zinc chloride (ZnCl2) is essential for converting grams of zinc to moles and subsequently determining the molarity of the resulting solution.

Recommended video:

Molar Mass Concept

Related Practice

To what volume should you dilute 50.0 mL of a 12 M stock HNO₃ solution to obtain a 0.100 M HNO₃ solution?

1716

views

Textbook Question

What is the minimum amount of 6.0 M H₂SO₄ necessary to produce 25.0 g of H₂(g) according to the reaction between aluminum and sulfuric acid? 2 Al(s) + 3 H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3 H₂(g)

Consider the reaction: Li₂S(aq) + Co(NO₃)₂(aq) → 2 LiNO₃(aq) + CoS(s) What volume of 0.150 M Li₂S solution is required to completely react with 125 mL of 0.150 M Co(NO₃)₂?

2484

views

Textbook Question

A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Pb(NO₃)₂(aq) → PbCl₂(s) + 2 KNO₃(aq) The solid PbCl₂ is collected, dried, and found to have a mass of 2.45 g. Determine the the percent yield.

3560

views

Textbook Question

A 55.0-mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K₂SO₄(aq) + Pb(C₂H₃O₂)₂(aq) → 2 KC₂H₃O₂(aq) + PbSO₄(s) The solid PbSO₄ is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, theoretical yield, percent yield.

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH₃OH c. Ca(NO₂)₂ d. C₆H₁₂O₆

1986

views

rank

What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl2(aq) → ZnCl2(aq) + Cu(s)

Verified Solution

Key Concepts

Molarity

Stoichiometry

Molar Mass

What is the molarity of ZnCl₂ that forms when 25.0 g of zinc completely reacts with CuCl₂ according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl₂(aq) → ZnCl₂(aq) + Cu(s)