A student sets up and solves the following equation to solve a problem in solution stoichiometry. Fill in the missing part of the student's equation. mol (6.9 (0.11 1) (119.86 = 91. g x10 μ

A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: H,SO, (aq) + BaCl, (aq) → Baso4 (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 39.5 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol • sulfuric acid = 98.0 g/mol

A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: 1H2SO4 (aq) +1 BaCl2 (aq) --> 1 BaSO4 (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 37.2 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? -g round your answer to appropriate significant digits. The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol sulfuric acid = 98.0 g/mol

3. Using the percentage equation given in the introduction, if 8.912 g of sand are recovered from an entire sand and salt mixture that weighed 10.4755 g. What was the percent of sand in the mixture?

A chemist adds 110.0 of a 1.63 molcalcium bromide (CaBr 2 ) solution to a reaction flask Calculate the mass in grams of calcium bromide the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

A chemist prepares a solution of silver(I) nitrate (AgNO,) by measuring out 245. µmol of silver(I) nitrate into a 400. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's silver(I) nitrate solution. Be sure your answer has the correct number of significant digits. u mol x10

Balance the following chemical equation and determine the number of moles of Fe(s) produced when 1 moles of Fe203(s) react with excess C(s) to produce Fe(s) and CO2(g). Fe203(s) + C(s) → Fe(s) + CO2(g) O Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105)

S + 6 HNO3 --> H₂SO4 + 6 NO2 + 2H₂O In the above equation how many moles of water can be made when 111.8 grams of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Sulfur 32 Oxygen 16

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A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. mol H 3.7 7 (0.22 L) (136.95 ) = L mol