(c) How many milliliters of 6.1 M HCl solution are needed to obtain 0.150 mol of HCl?

Verified step by step guidance

Determine the number of moles of HCl required, which is given as 0.150 mol.

Identify the concentration of the HCl solution, which is 6.1 M. This means there are 6.1 moles of HCl per liter of solution.

Use the formula for molarity: Molarity (M) = moles of solute / liters of solution. Rearrange this formula to solve for the volume of the solution: Volume (liters) = moles of solute / Molarity (M).

Convert the volume from liters to milliliters knowing that 1 liter = 1000 milliliters.

Calculate the volume of the 6.1 M HCl solution needed to obtain 0.150 mol of HCl using the rearranged molarity formula and the conversion factor.

Verified video answer for a similar problem:

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

Video duration:

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 calculating how much solute is present in a given volume of solution. Understanding molarity allows one to relate the amount of substance to the volume of solution, which is essential for solving dilution and concentration problems.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It allows chemists to predict how much of a substance is needed or produced in a reaction based on balanced chemical equations. In this context, stoichiometry helps in determining the volume of a concentrated solution required to achieve a specific number of moles of solute.

Volume Calculation

Volume calculation in chemistry often involves using the formula: Volume (L) = Moles of solute / Molarity. This relationship allows one to find the volume of a solution needed to provide a certain number of moles of solute. In this question, applying this formula will enable the calculation of the required volume of the 6.1 M HCl solution to obtain 0.150 mol of HCl.

Recommended video:

Guided course

02:35

Constant-Volume Calorimetry

Related Practice

Textbook Question

You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C12H22O11). (b) How many liters of water would you have to add to this solution to reduce the molarity you calculated in part (a) by a factor of two?

(b) How many moles of KBr are present in 150 mL of a 0.112 M solution?

963

views

Textbook Question

A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assuming no change in blood volume?

1210

views