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3.56d | Calculate the molarity: 0.0079 g C7H5SNO3 in one ounce (29.6 mL), the concentration of
3.56c | Calculate the molarity: 0.001 mg Cd2+ in 0.100 L, the maximum permissible concentration of
3.56a | Calculate the molarity: 293 g HCl in 666 mL of solution, a concentrated HCl solution
3.56b | Calculate the molarity: 2.026 g FeCl3 in 0.1250 L of a solution used as an unknown in
3.55a | Calculate the molarity: 0.195 g of cholesterol, C27H46O, in 0.100 L of serum, the average
3.48c | Determine the molarity: 20.54 g of Al(NO3)3 in 1575 mL of solution
3.52b | Calculate the mass: 75.0 mL of 2.2 × 10^−5 M H2SO4, a sample of acid rain
3.52d | Calculate the number of moles and the mass: 10.5 L of 3.716 M (NH4)2SO4, a liquid fertilizer
3.52a | Calculate the mass: 325 mL of 8.23 × 10^−5 M KI, a source of iodine in the diet
3.57 | There is about 1.0 g of calcium, as Ca2+, in 1.0 L of milk. What is the molarity of Ca2+ in
3.63b | Find the molarity: 0.5000 L of a 0.1222-M solution of C3H7OH is diluted to a final volume of
3.66 | An experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many
