. Sodium acetate can be formed from the metathesis/double replacement reaction of sodium bicarbonate and acetic acid. (See the Supplemental Information concerning metathesis reactions.) Determine the percent yield when 0.537 g of sodium acetate is obtained from mixing 15.0 g of NaHCO, with 125 mL of 0.15 M acetic acid.

You are in lab and ready to mix a beaker containing a solution of sodium cyanide with a beaker containing a solution of cobalt (III) acetate. You mix 45.0 mL of a 6.32 M solution of the sodium cyanide with an excess amount of cobalt (III) acetate. 1. Write out the balanced molecular reaction (including all physical states) for this reaction. 2. Calculate the amount of moles of sodium cyanide that was added into the mixture. 3. Calculate the minimum amount of moles of cobalt (III) acetate required to completely react the sodium cyanide. 4. Calculate the mass, in grams, of the solid produced from the reaction.

A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams of calcium oxide should the student obtain if his solution contains 53.0 mL of 0.461 M calcium nitrate?

With 85% H2SO4 by volume in water being used in the reaction, how many moles of water will be added to the reaction when 1.25 mL of 85% H2SO4 IS added ?

1. If 0.60 mol chlorine reacts with excess sodium, and 1.1 mol NaCl are produced, what is the percent yield for the reaction? 2. We need 35.0 mL of 0.3 M H2SO4 solution to completely titrate 22.00 mL of NaOH solution of unknown concentration.  What is the molarity of the sodium hydroxide solution?          H2SO4  + 2NaOH     Na2SO4   + 2H2O

3. You have dissolved 5 g of a rock containing a mixture of calcium carbonate and inert sand in 100 mL of 1 mol L-1 HCI. You measure the calcium concentration of the resulting solution as 0.03 mol L-1 in that 100 mL solution. Calculate the percentage calcium carbonate by weight in the rock sample.

200. mL of 2.50 M H2SO4 is added to 300. mL of 4.00 M H2SO4. Assuming that the volumes are additive, what is the final concentration?

What mass of solid product is formed when 50.0 mL of 0.10 M Pb(NO3)2 (aq) is mixed with 75.0 mL of 0.10 M NaCl (aq)? Assume a 100% yield. Thank you!

Barium can be analyzed by precipitating it as BaS04 and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H2S04, 0.0891 g of BaS04 formed. What percentage of barium is in the compound?

0.8888 g a mixture contains calcium chloride and potassium nitrate. To determine the % of each compound, silver nitrate was added to these solutions to precipitate all the chlorine in a form of silver chloride. 1.885 grams of silver chloride was precipitated, washed and dried. Calculate the % of calcium chloride in the sample.