Silver chloride, often used in silver plating, contains 75.27% Ag. Calculate the mass of silver chloride required to plate 205 mg of pure silver
Silver chloride, often used in silver plating, contains 75.27% Ag. Calculate the mass of silver chloride...
Silver Chloride, often used in silver plating, contains 75.27%AG. Caculate the mass of silver chloride required to plate 295 mg of pure silver.
Estimate molarity Estimate molarity of silver ions Ag^+ in a mixture that contains silver chloride AgCl and 10^-3 M KCI. K_sp (AgCl) = 1.8 times 10^-10.
Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon in an aqueous solution of silver cyanide, Ag(CN2. Label anode, cathode, direction of electron flow, and write the cathode half-reaction. Calculate the time required to plate 0.100 g of silver on a metal spoon using a current of 500 mA. (3 marks) Electrolysis is often used to electroplate metal objects. Sketch an electrolysis cell used to silver plate a metal spoon...
Show all work for full credit for problems 1-3. 1. Ibuprofen has the mass percent composition: carbon = 75.69%; hydrogen = 8.80% and oxygen 15.51%. Calculate the empirical formula. Answer: Pls answer all Questions thanks 2. How many grams of chlorine are in 22.50g of CF3C13? Answer: 3. Silver chloride, used in silver plating, contains 75.27% silver. Calculate the mass of silver chloride in grams required to make 4.8 g of silver metal. Answer: 4. Predict the products and write...
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ A.) Calculate ΔH for formation of 0.100 mol of AgCl by this reaction. I got A ΔH=-6.55 kJ B.) Calculate ΔH for the formation of 2.80 g of AgCl. C.) Calculate ΔH when 0.110 mmol of AgCl dissolves in water. Need help with B and C.
When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+(aq)+Cl−(aq)→AgCl(s)ΔH=−65.5kJ Calculate ΔH for formation of 0.490 mol of AgCl by this reaction. Calculate ΔH for the formation of 7.50 g of AgCl. Calculate ΔH when 9.23×10−4 mol of AgCl dissolves in water.
Why can a silver electrode be used as an indicator electrode for Ag^+ and halides? The silver electrode contains two membranes. One membrane contains a substance that reacts with Ag^+ and halides to form an ionic silver-halide complex. The potential difference created at the second, ion-selective membrane changes as the [silver-halide complex] changes. Because Ag^+ and halides equilibrate with ion-exchange sites at the outer surface of the ion-selective membrane. Diffusion of Ag^+ and halides out of the membrane creates a...
I need help with questions 3 and 4!! 3. Calculate the normality of the silver nitrate solution and percent chloride in the sample: 352.4 mg pure KCl require 48.33 ml AgNO3 solution 323.3 mg of unknown requires 32.02 ml AgNO3 solution Calculate the titration error. 4. A sample of silver alloy weighing 984.6 mg was dissolved in nitric acid. The solution was neutralized, and 252.2 mg of pure NaCl added. The excess chloride required 19.09 ml of 0.0935 N AgNO3...
Q7) A 1.23 g sample, which contains gold (Au), silver (Ag) and metal oxides, is treated with concentrated nitric acid (HNO;), which dissolves all the metals and metal oxides with the exception of the gold. The mass of yellow metal remaining is 7.4 x 10 g. The solution is then treated with aqueous sodium chloride (NaCI), which precipitates silver chloride (AgCI) and nothing else. A total of 0.196 g of AgCl is obtained. What is the percent gold and silver...
Commercial silver plating operations frequently use a solution containing the complex |Ag(CN)_2] ion. Because the formation constant K_f is quite large, this procedure ensures that the free Ag+ concentration in solution is low to promote uniform electrodeposition. In one process, a chemist added 9.0 L of 1.1M NaCN to 90.0 L of 0.12 M AgN0_3. Calculate the concentration of free Ag+ ions at equilibrium. K_f for this reaction is 1.0 times 10^21. Enter your answer in scientific notation.