You need to know the amount of NaCl.
To find the volume of AgNO3 solution needed, we first calculate the moles of NaCl using the molar ratio between AgNO3 and NaCl in the balanced chemical equation. Then, we use the molarity of the AgNO3 solution to determine the volume: moles of NaCl x (1 mol AgNO3 / 1 mol NaCl) x (1 L / 0.117 mol) x 1000 mL = volume in mL.
No, it is not recommended to store AgNO3 solution in copper vessels as copper can react with the silver nitrate and form copper nitrate, which can contaminate the solution and affect its stability. It is better to use glass or plastic containers for storing AgNO3 solution.
Discolored AgNO3 in the titration with KSCN may indicate the presence of impurities or decomposition of the solution. This can lead to inaccurate results in the titration as the discolored solution may not react as expected with KSCN. It is important to use a fresh and clear AgNO3 solution for accurate titration results.
They will form NaNO3 in aqueous solution, and AgOH would precipitate out of solution. AgNO3(aq) + NaOH(aq) --> AgOH(s) + NaNO3(aq) This is an example of a double displacement/replacement reaction.
Silver nitrate (AgNO3) can be used to distinguish between Cl- and SO4-2 ions. When AgNO3 is added to a solution containing chloride ions (Cl-), a white precipitate of silver chloride (AgCl) forms. In contrast, when AgNO3 is added to a solution containing sulfate ions (SO4-2), no visible precipitate is formed.
To find the volume of AgNO3 solution needed, we first calculate the moles of NaCl using the molar ratio between AgNO3 and NaCl in the balanced chemical equation. Then, we use the molarity of the AgNO3 solution to determine the volume: moles of NaCl x (1 mol AgNO3 / 1 mol NaCl) x (1 L / 0.117 mol) x 1000 mL = volume in mL.
Carbon tetrachloride does not react with silver nitrate (AgNO3) to form a white precipitate because it lacks an available chlorine atom for the reaction to occur. The reaction between carbon tetrachloride and silver nitrate would require the replacement of the chlorine atom by the silver ion from silver nitrate, but this reaction does not happen due to the unreactive nature of carbon tetrachloride.
They will form NaNO3 in aqueous solution, and AgOH would precipitate out of solution. AgNO3(aq) + NaOH(aq) --> AgOH(s) + NaNO3(aq) This is an example of a double displacement/replacement reaction.
yes
Four ions exist: Na+, Cl-, Ag+, (NO3)-; sodium chloride react with silver nitrate:NaCl + AgNO3 = AgCl + NaNO3AgCl is insoluble in water.
AgCl and KNO3.
alcl3+hno3
These compounds react forming a white insoluble precipitate - silver chloride: NaCl + AgNO3 = AgCl + NaNO3
155.0 mL x 0.274 M SO42- reacts with 155.0 x 0.274 * 2 (Ag+/SO42-) = 84.94 mmol Ag+84.94 mmol Ag+ is in 84.94 (mmolAg+) / 0.305 (M Ag+) = 84.94/0.305 = 278.5 mL of 0.305 M Ag+.Na+ and NO3- are tribuned out of this reaction.
Silver nitrate (AgNO3) can be used to distinguish between Cl- and SO4-2 ions. When AgNO3 is added to a solution containing chloride ions (Cl-), a white precipitate of silver chloride (AgCl) forms. In contrast, when AgNO3 is added to a solution containing sulfate ions (SO4-2), no visible precipitate is formed.
The net ionic equation for AgNO3 + HNO3 is: Ag+ + NO3- + H+ → AgNO3 + H+.
Ok, lets begin by writing out the reaction : 2AgNO3 +CaCl2 --> 2AgCl(s) + Ca(NO3)2 Precipitate = AgCl Now find the mol of compound in each solution: 14g AgNO3 x (mol/170g) = .082mol 4.83g CaCl2 x (mol/111g) = .044mol Determine limiting reactant: Notice in reaction that 2 CaCl2 molecules react with 1 AgNO3. Because 2(.044mol) > 1(.082mol), AgNO3 is your limiting reactant. Now that you know this you can find the mass of the precipitate .082molAgNO3x (2molAgCl/2molAgNO3)x(143.3g/molAgCl) = 11.75g b) Assuming all the AgNO3 is exhausted, there will be 2(.044)-(.082) = .006mol CaCl2 left .006mol x (111g/mol) = 0.67g CaCl2