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A 0.5711 g sample of a pure soluble chloride compound is dissolved in water, and all...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and...
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 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and...
A 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and treated with an excess of aqueous barium chloride, resulting in the precipitation of all the sulfate ion as barium sulfate. The precipitate was collected, dried, and found to weigh 2.3.3 g. Determine the atomic mass of M, and identify M.
A mixture consisting of only iron(III) chloride (FeCl3) and aluminum chloride (AlCl3) weighs 1.0397 g. When...
A mixture consisting of only iron(III) chloride (FeCl3) and aluminum chloride (AlCl3) weighs 1.0397 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the chloride ions associated with the original mixture are precipitated as insoluble silver chloride (AgCl). The mass of the silver chloride is found to be 3.0178 g. Calculate the mass percentages of iron(III) chloride and aluminum chloride in the original mixture. Mass percent FeCl3 = % Mass percent AlCl3...
A sample of a substance with the empirical formula XC1_2 weighs 0.5785 g. When it is...
A sample of a substance with the empirical formula XC1_2 weighs 0.5785 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2794 g. The chemical reaction is XCI_2 + 2 AgNO_3 rightarrow 2 AgCI + X(NO_3)_2 Calculate the formula mass of XCI_2. Formula mass XCI_2 = g mol^-1 Calculate the atomic mass of X. Atomic...
A 12.42 g sample of a mixture of NaClø and CaCl2ø) was dissolved in water. Excess...
A 12.42 g sample of a mixture of NaClø and CaCl2ø) was dissolved in water. Excess AgNO was added and all of the chloride was precipitated as AgCl. 31.70 g of AgCI was collected. Calculate the %w/w of NaCl in the original mixture.
A sample of a substance with the empirical formula XCl3 weighs 0.5183 g. When it is...
A sample of a substance with the empirical formula XCl3 weighs 0.5183 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCI by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to he 1.4071 g. The chemical reaction is XCl3 +3 AgNO3 3AgCI + X(NO3)3 (a) Calculate the formula mass of XCl3. Formula mass XCI3- g mol (b) Calculate the atomic mass of X Atomic mass X-...
The compound aluminum chloride is a strong electrolyte. Write the reaction when solid aluminum chloride is...
The compound aluminum chloride is a strong electrolyte. Write the reaction when solid aluminum chloride is put into water: Submit Answer Retry Entire Group 7 more group attempts remaining The compound silver nitrate is a strong electrolyte. Write the reaction when solid silver nitrate is put into water: Submit Answer Retry Entire Group 7 more group attempts remaining
6 b) In the laboratory a student combines 46.6 mL of a 0.322 M potassium sulfate...
6 b) In the laboratory a student combines 46.6 mL of a 0.322 M potassium sulfate solution with 19.0 mL of a 0.503 M cobalt(II) sulfate solution. What is the final concentration of sulfate anion ? M 18 a) A 0.5655 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide ion is precipitated as AgBr by the addition of an excess of silver nitrate. The mass of the resulting AgBr is found...
A sample of a substance with the empirical formula XCl3 weighs 0.4393 g. When it is...
A sample of a substance with the empirical formula XCl3 weighs 0.4393 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.1926 g. The chemical reaction is XCl3 + 3 AgNO33AgCl + X(NO3)3 (a) Calculate the formula mass of XCl3. Formula mass XCl3 = g mol-1 (b) Calculate the atomic mass of X. Atomic mass...
For the following reaction, 5.09 grams of iron(II) chloride are mixed with excess silver nitrate Assume...
For the following reaction, 5.09 grams of iron(II) chloride are mixed with excess silver nitrate Assume that the percent yield of iron(II) nitrate is 93.4% Iron(II) chloride(aq) + silver nitrate(aq) iron(II) nitrate(aq) + silver chloride(s) What is the ideal yield of iron(II) nitrate? What is the actual yield of iron(II) nitrate? grams grams Submit ANSWER Retry Entire Group 2 more group attempts remaining The equation for this reaction is: FeCl2(aq) + 2 AgNO3(aq) - Fe(NO3)2(aq) + 2 AgCl(s)
A 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and treated with an excess of aqueous barium chloride, resulting in the precipitation of all the sulfate ion as barium sulfate. The precipitate was collected, dried, and found to weigh 2.3.3 g. Determine the atomic mass of M, and identify M.
A sample of a substance with the empirical formula XC1_2 weighs 0.5785 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2794 g. The chemical reaction is XCI_2 + 2 AgNO_3 rightarrow 2 AgCI + X(NO_3)_2 Calculate the formula mass of XCI_2. Formula mass XCI_2 = g mol^-1 Calculate the atomic mass of X. Atomic...
A 12.42 g sample of a mixture of NaClø and CaCl2ø) was dissolved in water. Excess AgNO was added and all of the chloride was precipitated as AgCl. 31.70 g of AgCI was collected. Calculate the %w/w of NaCl in the original mixture.
A sample of a substance with the empirical formula XCl3 weighs 0.5183 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCI by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to he 1.4071 g. The chemical reaction is XCl3 +3 AgNO3 3AgCI + X(NO3)3 (a) Calculate the formula mass of XCl3. Formula mass XCI3- g mol (b) Calculate the atomic mass of X Atomic mass X-...
The compound aluminum chloride is a strong electrolyte. Write the reaction when solid aluminum chloride is put into water: Submit Answer Retry Entire Group 7 more group attempts remaining The compound silver nitrate is a strong electrolyte. Write the reaction when solid silver nitrate is put into water: Submit Answer Retry Entire Group 7 more group attempts remaining
For the following reaction, 5.09 grams of iron(II) chloride are mixed with excess silver nitrate Assume that the percent yield of iron(II) nitrate is 93.4% Iron(II) chloride(aq) + silver nitrate(aq) iron(II) nitrate(aq) + silver chloride(s) What is the ideal yield of iron(II) nitrate? What is the actual yield of iron(II) nitrate? grams grams Submit ANSWER Retry Entire Group 2 more group attempts remaining The equation for this reaction is: FeCl2(aq) + 2 AgNO3(aq) - Fe(NO3)2(aq) + 2 AgCl(s)
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