Skip to main content
Pearson+ LogoPearson+ Logo
Ch.5 - Introduction to Solutions and Aqueous Solutions
All textbooksTro 5th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 30
Chapter 5, Problem 30

If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?

Verified step by step guidance
1
Identify the initial conditions: the initial volume \( V_1 = 3.5 \) L and the initial molarity \( M_1 = 4.8 \) M.
Identify the final volume after dilution: \( V_2 = 45 \) L.
Use the dilution formula: \( M_1 \times V_1 = M_2 \times V_2 \), where \( M_2 \) is the molarity of the diluted solution.
Rearrange the formula to solve for \( M_2 \): \( M_2 = \frac{M_1 \times V_1}{V_2} \).
Substitute the known values into the equation: \( M_2 = \frac{4.8 \times 3.5}{45} \) to find the molarity of the diluted solution.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1m
Was this helpful?

Key Concepts

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

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L) and is crucial for understanding how much solute is present in a given volume of solution. Molarity is commonly used in chemistry to prepare solutions and perform stoichiometric calculations.
Recommended video:
Guided course
01:13
Molarity

Dilution

Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. The dilution equation, M1V1 = M2V2, relates the initial and final molarity (M) and volume (V) of the solution. This concept is essential for calculating the new concentration after a solution has been diluted.
Recommended video:
Guided course
00:58
Dilution Equation

Conservation of Moles

The conservation of moles principle states that the number of moles of solute remains constant before and after dilution, assuming no solute is added or removed. This principle underlies the dilution equation and allows for the calculation of the final concentration by equating the moles of solute in the initial and diluted solutions.
Recommended video:
Guided course
01:48
Law of Conservation of Mass
Related Practice
Textbook Question

A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?

Textbook Question

A chemist wants to make 5.5 L of a 0.300 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?

Textbook Question

If 123 mL of a 1.1 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?

1
views
Textbook Question

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

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)

1
views
Textbook Question

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?