**Chemical Reaction Problem**Calculate the mass of precipitate (in grams) formed when 20.5 mL of 0.300 M Ni(NO₃)₂ reacts with 16.0 mL of 0.300 M NaOH in the following chemical reaction:\[ \text{Ni(NO}_3\text{)}_2\text{(aq) + 2 NaOH(aq)} \rightarrow \text{Ni(OH)}_2\text{(s) + 2 NaNO}_3\text{(aq)} \]**Instructions for Calculation:**1. Determine the moles of each reactant: - Use the formula: \(\text{Moles} = \text{Molarity} \times \text{Volume (L)}\).2. Identify the limiting reactant: - Compare the mole ratio from the balanced equation to the moles calculated.3. Calculate the moles of \(\text{Ni(OH)}_2\) formed.4. Convert moles of \(\text{Ni(OH)}_2\) into grams: - Use the molar mass of \(\text{Ni(OH)}_2\) for the conversion.

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What mass of precipitate (in g) is formed when 20.5 mL of 0.300 M Ni(NO3)2 reacts with 16.0 mL of 0.300 M NaOH in the following chemical reaction? Ni(NO3)2(aq) + 2 NaOH(aq) →→→ Ni(OH)2(s) + 2 NaNO3(aq) h

What mass of precipitate (in g) is formed when 20.5 mL of 0.300 M Ni(NO3)2 reacts with 16.0 mL of 0.300 M NaOH in the following chemical reaction? Ni(NO3)2(aq) + 2 NaOH(aq) →→→ Ni(OH)2(s) + 2 NaNO3(aq) h

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

**Chemical Reaction Problem**

Calculate the mass of precipitate (in grams) formed when 20.5 mL of 0.300 M Ni(NO₃)₂ reacts with 16.0 mL of 0.300 M NaOH in the following chemical reaction:

\[ \text{Ni(NO}_3\text{)}_2\text{(aq) + 2 NaOH(aq)} \rightarrow \text{Ni(OH)}_2\text{(s) + 2 NaNO}_3\text{(aq)} \]

**Instructions for Calculation:**

1. Determine the moles of each reactant:
- Use the formula: \(\text{Moles} = \text{Molarity} \times \text{Volume (L)}\).

2. Identify the limiting reactant:
- Compare the mole ratio from the balanced equation to the moles calculated.

3. Calculate the moles of \(\text{Ni(OH)}_2\) formed.

4. Convert moles of \(\text{Ni(OH)}_2\) into grams:
- Use the molar mass of \(\text{Ni(OH)}_2\) for the conversion.

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