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Which has higher lattice energy AgCl and AgBr?
AgCl has a higher lattice energy than AgBr because Cl- is a smaller ion than Br-, resulting in stronger electrostatic interactions in AgCl.
What is the mole ratio of BaCl2 to AgCl?
The mole ratio of BaCl2 to AgCl is 1:2. This means that for every 1 mole of BaCl2, 2 moles of AgCl are produced in the chemical reaction.
How many moles is 573.28g of AgCl?
There's 4 moles.
Is AgCl soluble?
Yes, AgCl (silver chloride) has low solubility in water. It is sparingly soluble and forms a white precipitate when it is formed in solution.
If you had AgCl what state of matter would it be in?
AgCl, or silver chloride, is a white solid at room temperature.
Is AgCl solid or aqueous?
AgCl is highly insoluble, as it is a precipitate.
What is the chemical compound name for AgCl?
The chemical compound name for AgCl is silver chloride.
Which has higher lattice energy AgCl and AgBr?
AgCl has a higher lattice energy than AgBr because Cl- is a smaller ion than Br-, resulting in stronger electrostatic interactions in AgCl.
What is the mole ratio of BaCl2 to AgCl?
The mole ratio of BaCl2 to AgCl is 1:2. This means that for every 1 mole of BaCl2, 2 moles of AgCl are produced in the chemical reaction.
How many moles is 573.28g of AgCl?
There's 4 moles.
AgCl solid liquid or gas?
AgCl is a white crystalline solid and is well known for its low solubility in water.
Is AgCl soluble?
Yes, AgCl (silver chloride) has low solubility in water. It is sparingly soluble and forms a white precipitate when it is formed in solution.
What is the solubility of AgCl in a 0.35 M solution of NaCl?
(AgCl has Ksp = 1.8 x 10-10)-5.1 x 10-10
If you had AgCl what state of matter would it be in?
AgCl, or silver chloride, is a white solid at room temperature.
Can you separate AgCl from NaCl?
Yes, AgCl can be separated from NaCl by adding ammonia solution. AgCl is insoluble in ammonia, so it will precipitate out as a solid while NaCl remains in the solution. The two can then be filtered or separated by decantation.
How many grams of solid AgCl are needed to make 4.0 liters of a 5.0 M solution of AgCl?
To determine the mass of AgCl needed, first calculate the number of moles needed using the molarity equation: moles = molarity x volume (in L). Then, convert moles of AgCl to grams by using the molar mass of AgCl (107.87 g/mol for Ag and 35.45 g/mol for Cl). Finally, perform the calculation to find the grams of AgCl required.
Determine the solubility of AgCl from the following cell?
Need more info. AgCl, however, is very poorly soluble.
