Question

measuring concentration
molarity
______ is the amount of solute in a given amount of solvent or solution.
____ is a common measure of concentration. it is expressed in __ of solute per liter of ____.
you found the molarity of a solution containing 52 grams of sodium hydroxide. what would the solution’s molarity be if you instead had 80.0 grams naoh that was added to 200 milliliters of water?
______ m
how many grams of h₂so₄ are in a 500 - milliliter solution of 12.0 m h₂so₄?
______ grams
write the equation for diluting a solution:
using the equation, calculate the volume of 6.0 m hcl needed to create 250 milliliters of 0.10 m hcl.
______ ml
saturation
if a solution is saturated, then the solvent ( □can □cannot ) hold more solute in it.
if more solute is added to a solvent and stirred and it doesn’t dissolve, then it is ______.
if more solute is added to a solvent and stirred and it does dissolve after stirring, then it is ______.
if a solution is saturated, it can be made to hold more solute by ______ the temperature.
______ solution holds more solute than the solution normally should.
making a supersaturated solution requires you to ( □heat □cool ) the solution, add more solute, and then ( □heat □cool ) the solution.
a supersaturated solution tends to be highly ______. a supersaturated solution can easily become undissolved.
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Explanation:

1. Molarity of NaOH solution

Step1: Calculate moles of NaOH

Molar mass of NaOH is \(40\space g/mol\). Moles \(n=\frac{mass}{molar\space mass}=\frac{80.0\space g}{40\space g/mol}=2.0\space mol\)

Step2: Convert volume to liters

Volume of water is \(200\space mL = 0.2\space L\) (assuming solution volume is approximately solvent volume for dilute solutions)

Step3: Calculate molarity

Molarity \(M=\frac{n}{V}=\frac{2.0\space mol}{0.2\space L}=10.0\space M\) (Note: The original answer of 2.00 might have a miscalculation. Correcting here.)

2. Grams of \(H_2SO_4\)

Step1: Find moles of \(H_2SO_4\)

Molarity \(M = 12.0\space M\), Volume \(V=500\space mL = 0.5\space L\). Moles \(n = M\times V=12.0\space mol/L\times0.5\space L = 6.0\space mol\)

Step2: Calculate molar mass of \(H_2SO_4\)

Molar mass \(= 2\times1 + 32 + 4\times16=98\space g/mol\)

Step3: Find mass

Mass \(=n\times molar\space mass = 6.0\space mol\times98\space g/mol = 588\space g\)

3. Dilution equation

The dilution equation is \(M_1V_1 = M_2V_2\), where \(M_1,M_2\) are initial and final molarity, \(V_1,V_2\) are initial and final volume.

4. Volume of HCl for dilution

Step1: Identify values

\(M_1 = 6.0\space M\), \(M_2 = 0.10\space M\), \(V_2 = 250\space mL\)

Step2: Rearrange dilution equation

\(V_1=\frac{M_2V_2}{M_1}\)

Step3: Calculate \(V_1\)

\(V_1=\frac{0.10\space M\times250\space mL}{6.0\space M}\approx4.17\space mL\) (Note: The original answer of 0.47 is incorrect. Correcting here.)

5. Saturation questions

• If a solution is saturated, the solvent \(\boldsymbol{\text{cannot}}\) hold more solute.
• If more solute is added and it doesn’t dissolve, it is \(\boldsymbol{\text{saturated}}\).
• If it dissolves, it is \(\boldsymbol{\text{unsaturated}}\).
• A saturated solution can hold more solute by \(\boldsymbol{\text{increasing}}\) the temperature (for most solutes).
• A \(\boldsymbol{\text{supersaturated}}\) solution holds more solute than normal.
• To make a supersaturated solution, heat the solution, add solute, then cool it.
• Solute in supersaturated solution is highly \(\boldsymbol{\text{unstable}}\) and can become undissolved.

Answer:

s:

1. Molarity of NaOH solution: \(\boldsymbol{10.0\space M}\) (corrected)
2. Grams of \(H_2SO_4\): \(\boldsymbol{588\space g}\)
3. Dilution equation: \(\boldsymbol{M_1V_1 = M_2V_2}\)
4. Volume of HCl: \(\boldsymbol{\approx4.17\space mL}\) (corrected)
5. Saturation:

• cannot
• saturated
• unsaturated
• increasing
• supersaturated
• heat (first), cool (second)
• unstable