Question

Sodium hydroxide and magnesium chloride react as shown by this equation:
2NaOH + MgCl2 → Mg(OH)2 + 2NaCl.

Suppose the reaction begins with 637 milliliters of 1.35 M sodium hydroxide solution and excess magnesium hydroxide.

What is the theoretical yield of magnesium hydroxide if the resulting solution has a volume of 2.82 liters? Use the periodic table and the polyatomic ion resource.

The mass of magnesium hydroxide formed is ____ grams.

Answer 1

25.1 grams of magnesium Hydroxide are formed ..

Answer 2

The mass of magnesium hydroxide formed is 26 grams.

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in L)}}$    

Molarity of NaOH solution = 1.35 M

Volume of solution = 637 mL

Putting values in equation 1, we get:

$1.35M=\frac{\text{Moles of NaOH}\times 1000}{637}\\\\\text{Moles of NaOH}=0.90mol$

The balanced reaction is

$2NaOH+MgCl_2\rightarrow Mg(OH)_2+2NaCl$

2 moles of NaOH gives 1 mole of $Mg(OH)_2$

0.90  moles of NaOH give =$\frac{1}{2}\times 0.90=0.45$ moles of $Mg(OH)_2$

Mass of $Mg(OH)_2=moles\times {\text {molar mass}}=0.45mol\times 58g/mol=26g$

Learn more about stoichiometry

https://brainly.com/question/11083424

#learnwithbrainly