### Calculation of Calcium Bromide Solution ConcentrationA chemist prepares a solution of calcium bromide \((\text{CaBr}_2)\) by measuring out 17.0 g of calcium bromide into a 250 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's calcium bromide solution. Be sure your answer has the correct number of significant digits.**Answer Input:**- A box to input the concentration in mol/L.- Additional tools for calculation and help, such as a question mark icon for assistance.### Instructions:1. **Determine the Molar Mass of Calcium Bromide (\(\text{CaBr}_2\)):** - Calculate using the periodic table values for calcium (\(\text{Ca}\)) and bromine (\(\text{Br}\)).2. **Calculate the Number of Moles:** - Use the formula: \[ \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]3. **Determine the Molarity (Concentration in mol/L):** - Use the formula: \[ \text{molarity (mol/L)} = \frac{\text{moles of solute}}{\text{volume of solution (L)}} \] - Convert 250 mL to L by dividing by 1000.4. **Significant Figures:** - Ensure the final answer reflects the correct number of significant digits based on the given data.### Tools:- **Check Button:** To verify the answer.- **Save For Later:** To store progress.### Legal Notice:© 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Policy **Title: Preparing an Aqueous Potassium Dichromate Solution****Task:**A chemist must prepare 550. mL of 60.0 mM aqueous potassium dichromate \((K_2Cr_2O_7)\) working solution. The chemist achieves this by pouring out a specific volume of 0.403 mol/L aqueous potassium dichromate stock solution into a graduated cylinder and diluting it with distilled water.**Problem:**Calculate the volume in mL of the potassium dichromate stock solution that the chemist should pour out. Ensure your answer has the correct number of significant digits.**Interactive Elements:**- Input box labeled "mL" for the student to enter their calculated volume.- Functions to clear the input, undo entries, and request hints. **Notes:**Ensure calculations are accurate and check for significant figures. Use the equation for dilution: \[C_1V_1 = C_2V_2\]where \(C_1\) and \(V_1\) are the concentration and volume of the stock solution, respectively, and \(C_2\) and \(V_2\) are the desired concentration and volume of the working solution. **Options:**- **Check Button:** Submit your answer.- **Save For Later:** Save your progress to continue later.- **Submit Assignment:** Finalize your solution and complete the submission.*(No graphs or diagrams are included in this task.)*

The molarity of the solution is defined by the mole of solute present in one liter of solution. The molarity of a solution is calculated by the following formula: The mole of solute given by: Hence the molarity of the solution is given by:For the given solution: Molarity of the solution =? Mass of solute in gram is = 17. g The volume of the solution = 250. mL We know that the molar mass of CaBr2 is = 199.89 g/molLets put these values into the above formula:The concentration of CaBr2 solution is 0.34 mol/L. According to the guideline I solved one question and please put the second question in a separate session.