O Calculate the number of milliliters of 0.686 M Ba(OH)2 required to precipitate all of the Cu²+ ions in 171 mL of 0.502 M Cul2 solution as Cu(OH)2. The equation for the reaction is: Cul₂ (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + Bal₂ (aq) Volume = mL

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**Precipitation Reaction Calculation**

Calculate the number of milliliters of 0.686 M Ba(OH)₂ required to precipitate all of the Cu²⁺ ions in 171 mL of 0.502 M CuI₂ solution as Cu(OH)₂. 

The equation for the reaction is:

\[ \text{CuI}_2(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Cu(OH)}_2(s) + \text{BaI}_2(aq) \]

**Volume = [ ] mL**

In this experiment, you are tasked with determining the volume of barium hydroxide solution needed to completely precipitate copper ions from a copper(I) iodide solution, converting them into copper(II) hydroxide, a solid. Use the balanced chemical equation to understand the stoichiometry of the reaction, ensuring proper calculation of milliliters needed.
Transcribed Image Text:**Precipitation Reaction Calculation** Calculate the number of milliliters of 0.686 M Ba(OH)₂ required to precipitate all of the Cu²⁺ ions in 171 mL of 0.502 M CuI₂ solution as Cu(OH)₂. The equation for the reaction is: \[ \text{CuI}_2(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Cu(OH)}_2(s) + \text{BaI}_2(aq) \] **Volume = [ ] mL** In this experiment, you are tasked with determining the volume of barium hydroxide solution needed to completely precipitate copper ions from a copper(I) iodide solution, converting them into copper(II) hydroxide, a solid. Use the balanced chemical equation to understand the stoichiometry of the reaction, ensuring proper calculation of milliliters needed.
**Problem Statement:**

Calculate the volume (in mL) of a 0.773 M HNO₃ solution required to completely dissolve 8.42 g of MgCO₃.

**Chemical Reaction:**

\[ 2\text{HNO}_3(aq) + \text{MgCO}_3(s) \rightarrow \text{Mg(NO}_3\text{)}_2(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \]

**Solution Blank:**

\[ \boxed{\phantom{0000}} \text{ mL} \]
Transcribed Image Text:**Problem Statement:** Calculate the volume (in mL) of a 0.773 M HNO₃ solution required to completely dissolve 8.42 g of MgCO₃. **Chemical Reaction:** \[ 2\text{HNO}_3(aq) + \text{MgCO}_3(s) \rightarrow \text{Mg(NO}_3\text{)}_2(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \] **Solution Blank:** \[ \boxed{\phantom{0000}} \text{ mL} \]
Expert Solution
Step 1

a) given,

CuI2(aq) + Ba(OH)2 -----> Cu(OH)2(s) + BaI2(aq)

For Ba(OH)2 solution:

Concentration of Ba(OH)2 solution = 0.686 M = 0.686 mol/L

Volume of Ba(OH)2 solution = ?

For CuI2 solution:

Concentration of CuI2 solution = 0.502 M = 0.502 mol/L

Volume of CuI2 solution = 171 mL = 0.171 L

 

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