No. moles = mass/molecular mass mass of silver nitrate = 169.88
7.25/169.88 = 0.042 moles/l but this is per 100ml so we need to multiply by 10 = 0.42m
If the addition of excess silver nitrate precipitates 8.07 g silver chloride, the concentration of chloride ion in 229 mL solution is .25.
Mixing sea water with silver nitrate solution than a white solid called (Silver chlorie) AgCl will form. Sodium nitrate is also a product but it is dissolved in the water. AgNO3 + NaCl→AgCl + NaNO3
The silver in the Silver Nitrate precipitates the chloride ions out of the ammonium chloride solution, leaving Ammonium Nitrate in solution and a Silver Chloride solid.
The most common one is a solution of silver nitrate, which forms a white precipitate of silver chloride when added to a solution containing more than a minute concentration of chloride ions.
If the silver nitrate and ammonium chloride are both in solution when mixed, the very sparingly soluble silver chloride precipitates as a solid, leaving ammonium nitrate in the solution.
The number of moles of silver chromate formed will depend on the stoichiometry of the reaction between silver nitrate and potassium chromate. You need to know the balanced chemical equation, as well as the exact volumes and concentrations of the silver nitrate and potassium chromate solutions to calculate the number of moles of silver chromate formed.
If the addition of excess silver nitrate precipitates 8.07 g silver chloride, the concentration of chloride ion in 229 mL solution is .25.
0.3 Normality silver nitrate refers to a solution of silver nitrate (AgNO3) that has a concentration of 0.3 equivalents per liter (eq/L). This means that for every liter of the solution, there are 0.3 equivalents of silver nitrate present. The normality of a solution is a measure of the concentration of a solute in terms of equivalent weight.
Mixing sea water with silver nitrate solution than a white solid called (Silver chlorie) AgCl will form. Sodium nitrate is also a product but it is dissolved in the water. AgNO3 + NaCl→AgCl + NaNO3
No, you should not stir silver nitrate solution with a copper spoon because a chemical reaction will occur between the silver nitrate solution and the copper spoon, leading to the formation of solid silver. This will contaminate the solution and alter the experimental results.
No. Iron is a more reactive metal than silver, so the iron will replace the silver in the silver nitrate solution, forming an iron nitrate solution and solid silver. Eventually, the iron container will be gone, its atoms having gone into the iron nitrate solution.
They form Silver Iodide and Poassium nitrate. Silver Iodide is a yellow coloured compound which forms precipitate in the solution. Potassium Nitrate remains dissolved. These reactions only take place in solution. When both reactants are in solid state then reaction may not occur, or it is too slow to be observed.
The silver in the Silver Nitrate precipitates the chloride ions out of the ammonium chloride solution, leaving Ammonium Nitrate in solution and a Silver Chloride solid.
To find the concentration of the hydrochloric acid solution, you first need to convert the mass of the precipitate to moles using the molar mass of silver chloride. Then, use the mole ratio from the balanced chemical equation to find the moles of hydrochloric acid used. Finally, calculate the molarity by dividing the moles of hydrochloric acid by the volume in liters.
The transference number for silver ion (Ag+) in a 0.05 M silver nitrate solution is approximately 0.5, as it carries a single positive charge and has the same mobility as the nitrate ion (NO3-). The transference number for the nitrate ion in this solution is also around 0.5, implying that both ions move at similar rates under an electric field.
silver nitrate is a compound. it is not a mixture.
BeCl+AgN2+H2O----->BeN2+AgCl