The weight of CaF2 = 1.17 gm
Moles of CaF2 = 1.17 / 78.07 = 0.01498 Moles
Moles of Florine presents = 0.0299 Moles
Weight of Fluorine = 0.0299 x 18.99 = 0.5694 gm
% of Fluorine in the sample = 0.5694 x 100 /1.76 = 32.35 %
2. A compound containin ng uranium and fluorine weighed 1.760 grams and was treated with excess...
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed, dried, and weighed. The mass of the product (AgCl) is 0.4587 g. What is the wt% of Cl in the original sample? The molecular weight of AgCl is 143.32 g/mol.
What mass (g) of CaF 2 is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous calcium nitrate?
Impure sample of table salt that weighed 0.8421g, when dissolved in water and treated with excess AgNO3, formed 2.044g of AgCl. What is the percentage of NaCl in the impure sample? Do I need the molecular weight to start this equation? Where do I start?
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
A sample of ore containing manganese weighed 1.2354 grams. This sample was heated in a solution of nitric acid, which dissolved the manganese ion producing manganese(III) nitrate [Mn(NO3)3]. The acidity of the solution was adjusted, and hydrogen sulfide gas was bubbled into the solution producing 0.2876 grams of manganese(III) sulfide [Mn2S3]. What is the percentage of manganese in the original sample?
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2CO3. If the mass of the BaCO3 precipitate formed is 0.7578 g, what is the percent by mass of Ba in the original unknown compound?
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 0.47 g. What is the percentage by mass of NaNO3 in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer! Molar masses (in...
Question 2 If 6.2 grams of calcium nitrate, Ca(NO3)2, react with excess sodium phosphate, Na3PO4, according to 3Ca(NO3)2 + 2Na3PO4Ca3(PO4)2 + 6NaNO3 what is the theoretical yield of sodium nitrate, NaNO3, in grams? (Enter your answer to the hundredth nlace