Question

# 1. What is the percent of water in the hydrate of sodium acetate,

2. Borax is a powdery white hydrate that has been used as a cleaning product and pesticide for several decades. It has been determined that a 25.0g sample of borax contains 15.55g Borax and 9.45g H2O. Determine the % water in the borax hydrate to three sig figs?
3. What is the molarity of a 3.50 L solution containing 24.9 g of Li(NO3)? (MM Li(NO3) =68.951g)
4. How many grams of Ba(OH)2 would be needed to produce a 3.25 M solution with a volume of 0.750 L? (MM Ba(OH)2 = 171.346g)
5. What volume of solvent would be used in the preparation of a 1.75 M solution containing 33.7g of Sr(NO3)2? (MM Sr(NO3)2 = 211.64g)

A student performed a lab on a hydrate of calcium chloride (CaCl2). The data chart below shows a summary of the results from the experiment. Data Chart: Mass of test tube (g) 21.25 g Mass of test tube and hydrate (g) 24.38 g Mass of test tube and anhydrous material (g) 23.64 g
6. Calculate the mass of the hydrate.
7. Calculate the mass of the anhydrous material. 8. Calculate the mass of the water liberated.
9. Calculate the percent of water in the hydrate (this is the experimental value)
10. Calculate the moles of anhydrous material. The chemical formula for the anhydrous material is CaCl2. The formula mass of CaCl2 is 110.98 g.
11. Calculate the moles of water. The formula mass of water is 18.02 g.
12. Using your moles calculated in 5 and 6 determine the formula of the hydrate (round the number of waters to 3 sig figs NOT A WHOLE NUMBER).
13. Assuming that the correct formula of the hydrate is CaCl2 ∙ 2 H2O, what is the theoretical % of water in the hydrate? (round your % of water to 3 sig figs)
14. What is the percent error for the % of water in the hydrate of CaCl2 based on the experimental value (answer to number 4) and the theoretical value (answer to number 8)? (round your answer to 1 decimal place)

Step-by-step explanation
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