Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: How many milliliters of a 6.00 M NaOH solution are needed to provide 0.355 mol of NaOH?

Solution: How many milliliters of a 6.00 M NaOH solution are needed to provide 0.355 mol of NaOH?

Problem

How many milliliters of a 6.00 M NaOH solution are needed to provide 0.355 mol of NaOH?

Solution

We’re being asked to calculate the milliliter of 6.00 M NaOH needed to provide 0.355 mol NaOH solution.


The given values are:

Moles of NaOH needed = 0.355 mol NaOH

Molarity of NaOH = 6.00 M NaOH



Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters)

In other words:


Molarity(M)=moles of soluteLiters of solution


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