AgNO3reacts with Na3PO4as shown in the unbalanced equation below. How much mass of precipitate (Ag3PO4) would...
AgNO3reacts with Na3PO4as shown in the unbalanced equation below. How much mass of precipitate (Ag3PO4) would form when you react 25.0 mL of 0.500 M AgNO3and 5.00 mL of 2.00 M Na3PO4? (Hint—balance the chemical equation first)
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AgNO3reacts with Na3PO4as shown in the unbalanced equation
below. How much mass of precipitate (Ag3PO4) would...
1. When mixed, solutions of silver nitrate, AgNO, and sodium phosphate, Na3PO4, will form a precipitate...
1. When mixed, solutions of silver nitrate, AgNO, and sodium phosphate, Na3PO4, will form a precipitate of silver phosphate, Ag2PO4. The balanced equation is: 3AgNO3(aq) + Na3PO4(aq) Ag3PO4(s) + 3NaNO3(aq) Which of the following statements regarding this reaction is incorrect? A. 6 moles of AgNO, will react with 2 moles of Na2PO4 B. 9 moles of AgNO3 will form 2 moles of Ag3PO4, given sufficient Na3PO4 C. 1.5 moles of NaNO, will be formed when 0.5 mole of Na PO,...
Question 1 According to the following reaction, what mass of silver nitrate would be required to...
Question 1 According to the following reaction, what mass of silver nitrate would be required to react with 0.500 grams of potassium chloride? AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq) options 2.68 g 0.500 g 85.0 g 170 g 1.14 g Question 2 Consider the reaction: Na2CO3 (aq)+ 2 HCl (aq) --> 2 NaCl (aq) + CO2 (g) + H2O (l) If 43.41 g of sodium carbonate react completely, how many grams of HCl will be...
write a balanced equation including phases, and identifying the chemical formula of the precipitate. Part 1...
write a balanced equation including phases, and identifying
the chemical formula of the precipitate.
Part 1 - Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below. 1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. 2. A 50.0 ml graduated cylinder was then used to measure out 25.0 mL of 0.500...
a For the following unbalanced equation, indicate how many moles of the second reactant would be...
a For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.275 mol of the first reactant. Clz (9) + KI(aq) +1(8) + KCl(aq) mol KI b For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.355 mol of the first reactant. Co(s) +P$(s) + CogP2(8) mol P4 C For the following unbalanced equation, indicate how many moles of...
a For the following unbalanced equation, indicate how many moles of the second reactant would be...
a For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.275 mol of the first reactant. Cl2(g) + KI(aq) +12(8) + KCl(aq) mol KI b For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.355 mol of the first reactant. Co(s) +P(s) CozP2 (8) mol P4 C For the following unbalanced equation, indicate how many moles of the...
Hydrogen and oxygen react to form water vapor as seen in the unbalanced equation below. In...
Hydrogen and oxygen react to form water vapor as seen in the unbalanced equation below. In a 475 ml container at 533C, hydrogen has a pressure of 0.998 atm. Inside that vessel, oxygen is contained in a small tube with a volume of 25.0 ml, same temperature, and a pressure of 2.75 atm. The small vessel of oxygen is shattered and allowed to react according to the equation H2(g) + O2(g) - HO(g) What is the limiting reactant? What is...
Consider the unbalanced the equation given below for the of below CaH_33 (g) + O_2 rightarrow...
Consider the unbalanced the equation given below for the of below CaH_33 (g) + O_2 rightarrow CO_2(g) + H_2O Balance the equation and determine how many moles of O_2 are required to react completely with 4.9 moles of CaH_25? Consider the following general chemical equations 2A + 4B rightarrow 3C What is the theoretical yield of C when each of the initial quantities of A and B is allowed to react in the general equation a. 1.8 moles of A:...
10. Use the equation below to calculate the following. Ca(NO)2 (aq) Moles of NasPOs needed to...
10. Use the equation below to calculate the following. Ca(NO)2 (aq) Moles of NasPOs needed to react with 1.45 L of 0.225 M Ca(NOs) Balance the reaction. NasPO (aq) a. Cas(PO)2 (s) NaNOs (aq) b. c. Volume of 0.250 M Na PO4 needed to react with 15.00 mL of 0.500 M Ca(NOs)2 d. Grams of Cas(PO4)2 that can be obtained from 125 mlL of 0.500 M Ca(NO1) e. Molarity of Ca(NOs)2 when 40.00 mL react with 50.00 mL of 2.00...
HELP WITH B and C please ? (molarity stoich) How many grams of sodium nitrite are...
HELP WITH B and C please ? (molarity stoich)
How many grams of sodium nitrite are needed to make 2.50 L of 1.12 M solution? Calculate the number of moles of the precipitate formed when 525 mL of 0.500 M potassium iodide reacts with excess lead (II) nitrate. Balanced equation:___ Calculate the number of grams of precipitate formed when 2.00 L of 0.400 M calcium chloride reacts with excess silver nitrate. Balanced equation: How many milliliters of a 1.5 M...
1. (2 pts) A saline solution contains 1.1 % NaCl by mass. How much NaCl is...
1. (2 pts) A saline solution contains 1.1 % NaCl by mass. How much NaCl is present in 96.3 g of this solution? 2. (4 pts) How many liters of a 0.500 M sucrose (C12H22011) solution contains 1.5 kg of sucrose? 3. (2 pts) To what volume should you dilute 25 mL of a 12 M stock HCl solution to obtain a 0.500 M HCl solution? 4. (2 pts) Write the formula for the conjugate acid of the following bases:...
1. When mixed, solutions of silver nitrate, AgNO, and sodium phosphate, Na3PO4, will form a precipitate of silver phosphate, Ag2PO4. The balanced equation is: 3AgNO3(aq) + Na3PO4(aq) Ag3PO4(s) + 3NaNO3(aq) Which of the following statements regarding this reaction is incorrect? A. 6 moles of AgNO, will react with 2 moles of Na2PO4 B. 9 moles of AgNO3 will form 2 moles of Ag3PO4, given sufficient Na3PO4 C. 1.5 moles of NaNO, will be formed when 0.5 mole of Na PO,...
write a balanced equation including phases, and identifying
the chemical formula of the precipitate.
Part 1 - Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below. 1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. 2. A 50.0 ml graduated cylinder was then used to measure out 25.0 mL of 0.500...
a For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.275 mol of the first reactant. Clz (9) + KI(aq) +1(8) + KCl(aq) mol KI b For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.355 mol of the first reactant. Co(s) +P$(s) + CogP2(8) mol P4 C For the following unbalanced equation, indicate how many moles of...
a For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.275 mol of the first reactant. Cl2(g) + KI(aq) +12(8) + KCl(aq) mol KI b For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.355 mol of the first reactant. Co(s) +P(s) CozP2 (8) mol P4 C For the following unbalanced equation, indicate how many moles of the...
Hydrogen and oxygen react to form water vapor as seen in the unbalanced equation below. In a 475 ml container at 533C, hydrogen has a pressure of 0.998 atm. Inside that vessel, oxygen is contained in a small tube with a volume of 25.0 ml, same temperature, and a pressure of 2.75 atm. The small vessel of oxygen is shattered and allowed to react according to the equation H2(g) + O2(g) - HO(g) What is the limiting reactant? What is...
Consider the unbalanced the equation given below for the of below CaH_33 (g) + O_2 rightarrow CO_2(g) + H_2O Balance the equation and determine how many moles of O_2 are required to react completely with 4.9 moles of CaH_25? Consider the following general chemical equations 2A + 4B rightarrow 3C What is the theoretical yield of C when each of the initial quantities of A and B is allowed to react in the general equation a. 1.8 moles of A:...
10. Use the equation below to calculate the following. Ca(NO)2 (aq) Moles of NasPOs needed to react with 1.45 L of 0.225 M Ca(NOs) Balance the reaction. NasPO (aq) a. Cas(PO)2 (s) NaNOs (aq) b. c. Volume of 0.250 M Na PO4 needed to react with 15.00 mL of 0.500 M Ca(NOs)2 d. Grams of Cas(PO4)2 that can be obtained from 125 mlL of 0.500 M Ca(NO1) e. Molarity of Ca(NOs)2 when 40.00 mL react with 50.00 mL of 2.00...
HELP WITH B and C please ? (molarity stoich)
How many grams of sodium nitrite are needed to make 2.50 L of 1.12 M solution? Calculate the number of moles of the precipitate formed when 525 mL of 0.500 M potassium iodide reacts with excess lead (II) nitrate. Balanced equation:___ Calculate the number of grams of precipitate formed when 2.00 L of 0.400 M calcium chloride reacts with excess silver nitrate. Balanced equation: How many milliliters of a 1.5 M...
1. (2 pts) A saline solution contains 1.1 % NaCl by mass. How much NaCl is present in 96.3 g of this solution? 2. (4 pts) How many liters of a 0.500 M sucrose (C12H22011) solution contains 1.5 kg of sucrose? 3. (2 pts) To what volume should you dilute 25 mL of a 12 M stock HCl solution to obtain a 0.500 M HCl solution? 4. (2 pts) Write the formula for the conjugate acid of the following bases:...
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