The density of a solution is measured six times with results of 1.098, 1.100, 1.089, 1.095, 1.097, and 1.101 g/mL. Calculate the 95% confidence interval for the density. Refer to Table 4-4 for values of Student's t. O 1.0967 ± 0.004₁ g/mL O 1.0967 ± 0.0043 g/mL O 1.0967±0.0038 g/mL O 1.0967 ± 0.0045 g/mL O 1.0967 ± 0.0039 g/mL

6-40 What is the molarity of each solution? (a) 47 g of KCI dissolved in enough water to give 375 mL of solution (b) 82.6 g of sucrose, C12H22O11, dissolved in enough water to give 725 mL of solution (c) 9.3 g of ammonium sulfate, (NH4)2SO4 dissolved in enough water to give 2.35 L of solution

Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration of hydrogen in the palladium depends on the pressure of H2 gas applied, but in a more complex fashion than can be described by Henry's law. Under certain conditions, 0.94 g of hydrogen gas is dissolved in 215 g of palladium metal (solution density = 10.8 g cm3). (a) Determine the molarity of this solution. (b) Determine the molality of this solution. (c) Determine the percent by mass of hydrogen atoms in this solution.