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How many mol of AgCl can be precipitated by adding a solution containing 0.100 mol of AgNO3 to a solution containg excess NaCl?
One mole of AgNO3 reacts with one mole of NaCl to form one mole of AgCl precipitate. Therefore, 0.100 mol of AgNO3 will form 0.100 mol of AgCl precipitate when reacted with excess NaCl.
What volume of 0.131 M BaCl2 is required to react completely with 42.0 ml of .453 MNa2SO4. This is the net ionic equation for the reaction. Ba2 plus plus SO42---- BaSO4. Correct answer equals 145 ML?
first of all, you need to recognize that one mole of Na2SO4 is reacting with one mole of BaCL2. so find the moles of the NaSO4, then you automatically have the moles of the BaCL2. if you get the moles of the BaCL2, its easy to calculate the volume of it because you already have the MOLARITY. good luck
An impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgNO3 formed 2.044 g of Ag-Cl what is the percentage of Na-Cl in the impure sample?
2.044 g AgCl / 143.33 g per mole = 0.01426 moles of AgClNaCl + AgNO3 --> AgCl + NaNO31 mole of AgCl = 1 mole of NaClThe sample contained 0.01426 moles of NaCl0.01426 moles NaCl x 58.44 g per mole = 0.8334 g NaCl0.8334 / 0.8421 = 98.97% pureI'm pretty sure this is the correct answer.
4.02 grams of AgNO3 react with excess NaCl how many grams of silver nitrate are produced?
AgNo3(aq) + NaCl(aq) -------------->AgCl (ppt) + No3(-) + Na(+) no silver nitrates are produced it is all consumed. only silver chloride is produced and precipitate . free nitrate and free sodium ions are produced but do not react with each other 1 Mole AgNo3 ------->169.9 gm 1 Mole Nacl ------->58.4 gm 1 Mole AgCl ------->143.3 gm 4.02 gm AgNO3 = (4.02 / 169.9) = 0.02366 M AgCl produced = 0.02366 M = 3.39 gm
How do you make BaCl2 solution?
To make a BaCl2 (barium chloride) solution, first weigh out the appropriate amount of BaCl2 powder. Then dissolve it in a known volume of water, making sure the BaCl2 is completely dissolved. Finally, dilute the solution to reach the desired concentration, if needed.
When agno3 reacts with bacl2 agcl and bano32 are formed how many grams of agcl are formed when 10.0g of silver nitrate reacts with 15.0g of bacl2?
To find the amount of AgCl formed, we first need to calculate the limiting reagent. This is done by converting the given masses of AgNO3 and BaCl2 to moles, determining the mole ratio between them, and then the limiting reagent based on the smaller value. Once the limiting reagent is determined, use the mole ratio from the balanced chemical equation to find the moles of AgCl formed and then convert that to grams.
How many mol of AgCl can be precipitated by adding a solution containing 0.100 mol of AgNO3 to a solution containg excess NaCl?
One mole of AgNO3 reacts with one mole of NaCl to form one mole of AgCl precipitate. Therefore, 0.100 mol of AgNO3 will form 0.100 mol of AgCl precipitate when reacted with excess NaCl.
What is the formula of a hydrate that is 85.3 percent barium chloride and 14.7 percent water?
The formula of the hydrate is BaCl2•2H2O. The ratio of barium chloride to water is 1:2, so there are two moles of water for every mole of barium chloride in the compound.
What is the balanced equation of barium chloride and sodium chromate?
The balanced equation for the reaction between barium chloride (BaCl2) and sodium chromate (Na2CrO4) is: BaCl2 + Na2CrO4 -> BaCrO4 + 2NaCl
What volume of 0.131 M BaCl2 is required to react completely with 42.0 ml of .453 MNa2SO4. This is the net ionic equation for the reaction. Ba2 plus plus SO42---- BaSO4. Correct answer equals 145 ML?
first of all, you need to recognize that one mole of Na2SO4 is reacting with one mole of BaCL2. so find the moles of the NaSO4, then you automatically have the moles of the BaCL2. if you get the moles of the BaCL2, its easy to calculate the volume of it because you already have the MOLARITY. good luck
How many moles of AgCl will be produced from 83.0 g of AgNO3 assuming NaCl is available in excess?
The balanced chemical equation for this reaction is: AgNO3 + NaCl -> AgCl + NaNO3 From this equation, we can see that 1 mole of AgNO3 produces 1 mole of AgCl. Since the molar mass of AgNO3 is 169.87 g/mol, 83.0 g of AgNO3 is equivalent to 0.488 moles. Therefore, 0.488 moles of AgCl will be produced.
An impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgNO3 formed 2.044 g of Ag-Cl what is the percentage of Na-Cl in the impure sample?
2.044 g AgCl / 143.33 g per mole = 0.01426 moles of AgClNaCl + AgNO3 --> AgCl + NaNO31 mole of AgCl = 1 mole of NaClThe sample contained 0.01426 moles of NaCl0.01426 moles NaCl x 58.44 g per mole = 0.8334 g NaCl0.8334 / 0.8421 = 98.97% pureI'm pretty sure this is the correct answer.
What is the empirical formula of a compound that contains 75 percent Ag and 25 percent Cl by mass?
The empirical formula of the compound would be AgCl, as the ratio of silver to chlorine in the compound is 3:1 based on the given mass percentages (75% Ag and 25% Cl). This ratio simplifies to AgCl when expressed in the simplest whole number ratio.
4.02 grams of AgNO3 react with excess NaCl how many grams of silver nitrate are produced?
AgNo3(aq) + NaCl(aq) -------------->AgCl (ppt) + No3(-) + Na(+) no silver nitrates are produced it is all consumed. only silver chloride is produced and precipitate . free nitrate and free sodium ions are produced but do not react with each other 1 Mole AgNo3 ------->169.9 gm 1 Mole Nacl ------->58.4 gm 1 Mole AgCl ------->143.3 gm 4.02 gm AgNO3 = (4.02 / 169.9) = 0.02366 M AgCl produced = 0.02366 M = 3.39 gm
How do you figure out how much NaCl will be necessary to precipitate silver?
One mole of chloride (Cl-) to one mole of Ag+ ions: Cl- + Ag+ --> AgCl(s)
How do you make BaCl2 solution?
To make a BaCl2 (barium chloride) solution, first weigh out the appropriate amount of BaCl2 powder. Then dissolve it in a known volume of water, making sure the BaCl2 is completely dissolved. Finally, dilute the solution to reach the desired concentration, if needed.
Is silver chloride AgCl a mixture?
No, silver chloride (AgCl) is not a mixture. It is a compound composed of silver and chlorine atoms chemically bonded together in a fixed ratio.
