(a)
Interpretation:
The number of moles of each ion in the given solution is to be calculated.
Concept Introduction:
The
The number of moles is calculated by the formula,
The molarity is calculated by the formula,
Answer to Problem 50QAP
The number of moles of
Explanation of Solution
It is given that
The conversion of units of volume into
The number of moles of a solute is calculated by the formula,
Substitute the values of volume of solution and molarity of
The compound
Thus, the number of moles of
The number of moles of
Therefore, the number of moles of
(b)
Interpretation:
The number of moles of each ion in the given solution is to be calculated.
Concept Introduction:
The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.
The number of moles is calculated by the formula,
The molarity is calculated by the formula,
Answer to Problem 50QAP
The number of moles of
Explanation of Solution
It is given that
The number of moles of a solute is calculated by the formula,
Substitute the values of volume of solution and molarity of
The solution of
Thus, the number of moles of
The number of moles of
Therefore, the number of moles of
(c)
Interpretation:
The number of moles of each ion in the given solution is to be calculated.
Concept Introduction:
The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.
The number of moles is calculated by the formula,
The molarity is calculated by the formula,
Answer to Problem 50QAP
The number of moles of
Explanation of Solution
It is given that
The conversion of units of volume into
The number of moles of a solute is calculated by the formula,
Substitute the values of volume of solution and molarity of
The solution of
Thus, the number of moles of
The number of moles of
Therefore, the number of moles of
(d)
Interpretation:
The number of moles of each ion in the given solution is to be calculated.
Concept Introduction:
The atomic mass of an element is defined as the sum of number of protons and number of neutrons. Molar mass of an element is determined from atomic mass of an element.
The number of moles is calculated by the formula,
The molarity is calculated by the formula,
Answer to Problem 50QAP
The number of moles of
Explanation of Solution
It is given that
The conversion of units of volume into
The number of moles of a solute is calculated by the formula,
Substitute the values of volume of solution and molarity of
The solution of
Thus, the number of moles of
The number of moles of
Therefore, the number of moles of
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Chapter 15 Solutions
Introductory Chemistry: A Foundation
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- When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.arrow_forwardCalculate the number of moles and the mass of the solute in each of the following solutions: (a) 2.00 L of 18.5MH2SO4, concentrated sulfuric acid (b) 100.0 mL of 3.8105MNaCN, the minimum lethal concentration of sodium cyanide in blood serum (c) 5.50 L of 13.3 MH2CO, the formaldehyde used to fix tissue samples (d) 325 mL of 1.8106MFeSO4, the minimum concentration of iron sulfate detectable by taste in drinking waterarrow_forwardWhen a solution is diluted by adding additional solvent, the concentration of solute changes hut the amount of solute present does not change. Explain. Suppose 250. mL of water is added to 125 mL of 0.55 1 M NaCl solution. Explain how you would calculate the concentration of the solution after dilution.arrow_forward
- What is the difference between a solute and a solvent?arrow_forwardDetermine the molarity of each of the following solutions: (a) 1.457 mol KCl in 1.500 L of solution (b) 0.515 g of H2SO4 in 1.00 L of solution (c) 20.54 g of Al( NO3)3 in 1575 mL of solution (d) 2.76 kg of CuSO45H2O in 1.45 L of solution (e) 0.005653 mol of Br2 in 10.00 mL of solution (f) 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solutionarrow_forward3.64 How many grams of solute are present in each of these solutions? (a) 37.2 mL ofO.471 M HBr (b) 113.0 L of 1.43 M Na2CO3 (c) 212 mL of 6.8 M CH3COOH (d) 1.3 × 10-4 L of 1.03 M H2S03arrow_forward
- It took 25.06 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 79). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass.arrow_forwardThe units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2Oarrow_forwardCitric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?arrow_forward
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