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Dilution of Concentrated Solutions The number of moles of solute in V liters of a solution of molarity M is given by molessolute=MV It is often of practical importance to take a concentrated solution of known concentration, and to add solvent to it to obtain a diluted solution with a desired concentration. During the process of dilution, since only solvent is added, the number of moles of solute is constant. Using c to denote the concentrated solution, and d to denote the diluted solution, this becomes McVc=MdVd If three of the above quantities are known, then it is possible to solve for the fourth quantity. Note that any consistent set of volume units may be used in this equation, since the conversion factor from one unit to the other appears on both sides of the equation and will cancel out. In the laboratory, a student dilutes 10.4mL of a 9.13M hydrobromic acid solution to a total volume of 300.0mL. What is the concentration of the diluted solution? Concentration = M How many milliliters of 8.96M hydrobromic acid solution should be used to prepare 4.50L of 0.700MHBr ? mL In the laboratory, a student adds 46.7mL of water to 17.5mL of a 0.745M hydroiodic acid solution. What is the concentration of the diluted solution? Assume the volumes are additive. Concentration = M