For this one, Could someone check my work?(adsbygoogle = window.adsbygoogle || []).push({});

1.What volume of a 15.0mol/L standard solution of hydrochloric acid will be required a make a 450mL of a 2.25mol/L dilution?

[tex]\frac{15mol/L}{2.25mol/L}=6.67[/tex] *I think there is no unit for 6.67

[tex]=(6.67)(0.450L)=3L[/tex]

2.Will it be possible for you to produce 850mL of a 1.85mol/L acetic acid sloution if all you left in your orginal 7.50mol/L standard solution bottle is 200mL?

These long questions just confuse me. I don't know where to start on this question.

3.Consider the following acid-base reaction:

H_{2}SO_{4(aq)}+ Mg(OH)_{2(aq)}-------> MgSO_{4(aq)}+ 2H_{2}O_{(l)}

a) Determine how many grams of magnesium hydroxide you would need to add to water in order to obtain 5.50L of a 2.25mol/L magnesium hydroxide solution.

[tex]\frac{5.50L}{2.25mol/L}=2.44mol[/tex] *Molar mass for Mg(OH)_{2(aq)}is 58.31968g

[tex]2.44mol[/tex] x [tex] (\frac{58.32g}{1mol})=142.3g[/tex]

b)Suppose you had 6.00L of a 3.15mol/L sulfuric acid solution and 4.50L of a 7.00mol/L magnesium hydroxide solution. Which one of these would be the limiting reangent? How much of the excess reangent will be left unreacted?

[tex]\frac{6.00L}{3.15mol/L}=1.94mol [/tex] - Sulfuric Acid Solution

[tex]\frac{4.50L}{7.00mol/L}=0.64mol [/tex] - Magnesium Hydroxide Solution

I say the limiting reangent is the magnesium hydroxide solution and 1.3mol of sulfuric acid solution will remain unreacted.

c)Using the volumes and concentrations for part (b), how many grams of water will the reaction produce?

1.3mol *Molar mass ofH_{2}SO_{4(aq)}is 98.03g

[tex]1.30mol[/tex] x [tex] (\frac{98.03g}{1mol})=127.44g[/tex]

Please please check my work. It is worth a lot of marks.

Thank You

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# Homework Help: 3 Questions on Grd11 Chem

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