**Chemical Reaction Precipitation Calculation**In this example, we are tasked with determining the mass of the precipitate formed in a chemical reaction. The reaction involves:- 20.5 mL of 0.300 M Nickel(II) nitrate [Ni(NO₃)₂]- 33.5 mL of 0.300 M Sodium hydroxide (NaOH)The balanced chemical equation for the reaction is:\[ \text{Ni(NO}_3\text{)}_2(aq) + 2 \text{NaOH}(aq) \rightarrow \text{Ni(OH)}_2(s) + 2 \text{NaNO}_3(aq) \]Based on this equation, Nickel(II) hydroxide [Ni(OH)₂] is formed as a solid precipitate.**Steps:**1. **Calculate the Moles of Reactants:** - Use the molarity and volume of each solution to find moles. - \( \text{Moles of Ni(NO}_3\text{)}_2 = 0.300 \, \text{M} \times 0.0205 \, \text{L} \) - \( \text{Moles of NaOH} = 0.300 \, \text{M} \times 0.0335 \, \text{L} \)2. **Determine the Limiting Reactant:** - Compare stoichiometric ratios to determine which reactant limits the formation of Ni(OH)₂.3. **Calculate Mass of Precipitate:** - Use the moles of the limiting reactant to find the moles of Ni(OH)₂. - Determine the mass using the molar mass of Ni(OH)₂.An input field is shown at the bottom with a numeric keypad to enter the mass of the precipitate in grams.

Precipitate is a solid compound that is left over in a reaction. Molar mass is the mass of 1 mole…

Whát masŠ of precipitate (In g) Is formed when 20.5 mL of 0.300 Ni(NO3)2 reacts with 33.5 mL of 0.300 M NaOH in the following chemical reaction? Ni(NO3)2(aq) + 2 N2OH(aq) → Ni(OH).(s) + 2 NaNO.(aq)

Whát masŠ of precipitate (In g) Is formed when 20.5 mL of 0.300 Ni(NO3)2 reacts with 33.5 mL of 0.300 M NaOH in the following chemical reaction? Ni(NO3)2(aq) + 2 N2OH(aq) → Ni(OH).(s) + 2 NaNO.(aq)

Chemistry

10th Edition

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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