STARTING AMOUNT X How many gram of Cal: are needed to completely precipitate the Ag+ ions as Agl from 75.0 mL solution of 0.300 M AgNO, according to the balanced chemical reaction: 2 AgNO:(aq) + Cal:(aq) → 2 Agl(s) + Ca(NO3)2(aq) 2.64 ADD FACTOR x() 100 3.31 0.1 6.022 x 10² 293.89 1 0.01 LAgNO mol AgNO L solution 2 0.001 g Calz g AgNO, ANSWER 1.85 75.0 234.77 L Calz 164.09 1000 169.87 ml Cala mL AgNOs RESET 2 10 0.300 1.91 mol Calz
STARTING AMOUNT X How many gram of Cal: are needed to completely precipitate the Ag+ ions as Agl from 75.0 mL solution of 0.300 M AgNO, according to the balanced chemical reaction: 2 AgNO:(aq) + Cal:(aq) → 2 Agl(s) + Ca(NO3)2(aq) 2.64 ADD FACTOR x() 100 3.31 0.1 6.022 x 10² 293.89 1 0.01 LAgNO mol AgNO L solution 2 0.001 g Calz g AgNO, ANSWER 1.85 75.0 234.77 L Calz 164.09 1000 169.87 ml Cala mL AgNOs RESET 2 10 0.300 1.91 mol Calz
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
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![**Stoichiometry Problem: Precipitation Reaction**
**Problem Statement:**
Determine the number of grams of calcium (CaI₂) needed to completely precipitate the silver ions (Ag⁺) as silver iodide (AgI) from a 75.0 mL solution of 0.300 M AgNO₃ according to the balanced chemical reaction:
\[ 2 \, \text{AgNO}_3(\text{aq}) + \text{CaI}_2(\text{aq}) \rightarrow 2 \, \text{AgI}(\text{s}) + \text{Ca(NO}_3\text{)}_2(\text{aq}) \]
**Calculation Setup:**
The solution setup involves determining the starting amount and applying conversion factors to find the required mass of calcium iodide.
**Interface Elements Explained:**
- **Starting Amount Box:** Placeholder for inputting the initial substance quantity.
- **Conversion Factor Section:** Engages a set of brackets for multiplying by necessary conversion factors (e.g., molarity, molar mass).
- **Add Factor Button:** Buttons for selecting various factors like molar mass, volume, etc., are provided.
- **Answer and Reset Buttons:** Options to calculate or reset the input fields.
**Factors and Units:**
- Numerical factors such as 100, 6.022x10²³, 234.77, and others are likely values for molar calculations.
- Units involve L AgNO₃, mol AgNO₃, g CaI₂, among others, crucial for inter-conversion.
**Procedure Overview:**
1. **Starting Calculation:** Input the initial volume and concentration of AgNO₃.
2. **Apply Stoichiometry:** Follow the balanced equation to relate moles of AgNO₃ to mass of CaI₂.
3. **Result Interpretation:** Use the calculation tools to determine the mass of CaI₂ required.
This interactive tool supports students in visualizing and calculating stoichiometric relationships in precipitation reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ebf2b47-0653-48b1-aa4f-9532848d4742%2F8867bb5c-5005-44fe-8a15-a71b249dde2a%2Fv0nar5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Stoichiometry Problem: Precipitation Reaction**
**Problem Statement:**
Determine the number of grams of calcium (CaI₂) needed to completely precipitate the silver ions (Ag⁺) as silver iodide (AgI) from a 75.0 mL solution of 0.300 M AgNO₃ according to the balanced chemical reaction:
\[ 2 \, \text{AgNO}_3(\text{aq}) + \text{CaI}_2(\text{aq}) \rightarrow 2 \, \text{AgI}(\text{s}) + \text{Ca(NO}_3\text{)}_2(\text{aq}) \]
**Calculation Setup:**
The solution setup involves determining the starting amount and applying conversion factors to find the required mass of calcium iodide.
**Interface Elements Explained:**
- **Starting Amount Box:** Placeholder for inputting the initial substance quantity.
- **Conversion Factor Section:** Engages a set of brackets for multiplying by necessary conversion factors (e.g., molarity, molar mass).
- **Add Factor Button:** Buttons for selecting various factors like molar mass, volume, etc., are provided.
- **Answer and Reset Buttons:** Options to calculate or reset the input fields.
**Factors and Units:**
- Numerical factors such as 100, 6.022x10²³, 234.77, and others are likely values for molar calculations.
- Units involve L AgNO₃, mol AgNO₃, g CaI₂, among others, crucial for inter-conversion.
**Procedure Overview:**
1. **Starting Calculation:** Input the initial volume and concentration of AgNO₃.
2. **Apply Stoichiometry:** Follow the balanced equation to relate moles of AgNO₃ to mass of CaI₂.
3. **Result Interpretation:** Use the calculation tools to determine the mass of CaI₂ required.
This interactive tool supports students in visualizing and calculating stoichiometric relationships in precipitation reactions.
Expert Solution
Step 1
Calcium iodide reacts with silver nitrate to form calcium nitrate and precipitate of silver iodide. The balanced chemical reaction is as follows:
The stoichiometry of the balanced chemical reaction states that one mole of calcium iodide reacts with two moles of silver nitrate.
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