Calculate the mass, in grams, of potassium iodide that must be added to a 125-mL volumetric flask in order to prepare 125 mL of a 0.143 M aqueous solution of the salt. grams
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
i just need answers no explantion
![**Problem Statement:**
Calculate the mass, in grams, of **potassium iodide** that must be added to a **125-mL** volumetric flask in order to prepare **125 mL** of a **0.143 M** aqueous solution of the salt.
**Input Box:**
[_____] grams
---
**Explanation:**
This question aims to apply concepts from chemistry, specifically molarity and solution preparation. You are tasked to determine the mass of potassium iodide (KI) needed to create a specific molar concentration in a given volume of solution.
**Key Points:**
- **Molarity (M)** is defined as the number of moles of solute per liter of solution.
- The volume needed is 125 mL, which is equivalent to 0.125 L.
- The desired molarity of the potassium iodide solution is 0.143 M.
**Steps for Solution:**
1. Use the formula for molarity:
\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
\]
2. Calculate the number of moles of potassium iodide required:
\[
\text{moles of KI} = \text{Molarity} \times \text{Volume in liters}
\]
3. Convert moles to grams using the molar mass of potassium iodide (approximately 166 g/mol).
**Note:**
This exercise reinforces calculation skills in chemistry, specifically focusing on solution preparation and understanding molarity.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7b5abf62-aefa-4d0f-b576-4023d749f637%2F7be79a39-2433-43c6-9355-39e148e4bcb5%2Fzrriit_processed.png&w=3840&q=75)
![In the laboratory, a student adds 14.2 g of copper(II) iodide to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of copper(II) iodide, the copper(II) ion, and the iodide ion in the solution.
\[[\text{CuI}_2] = \_\_\_\_\ M\]
\[[\text{Cu}^{2+}] = \_\_\_\_\ M\]
\[[\text{I}^-] = \_\_\_\_\ M\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7b5abf62-aefa-4d0f-b576-4023d749f637%2F7be79a39-2433-43c6-9355-39e148e4bcb5%2Fmm3k94_processed.png&w=3840&q=75)
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