Silver nitrate calculating mass

In 1865 a chemist reported that he had reacted a weighed amoimt of pure silver with nitric acid and had recovered aU the silver as pure silver nitrate. The mass ratio of silver to silver nitrate was foimd to be 0.634985. Using only this ratio and the presently accepted values for the atomic weights of silver and oxygen, calculate the atomic... 

The concentration of Cl- ions can be measured gravimetrically by precipitating silver chloride, with silver nitrate as the precipitating reagent in the presence of dilute nitric acid. The white precipitate is filtered off and its mass is determined, (a) Calculate the Cl ion concentration in 25.00 mL of a solution that gave a silver chloride precipitate of mass 3.050 g. (b) Why is the method inappropriate for measuring the concentration of fluoride ions ... 

Silver chromate, Ag2Cr04, is insoluble. It forms a brick-red precipitate. Calculate the mass of silver chromate that forms when 50.0 mL of 0.100 mol/L silver nitrate reacts with 25.0 mL of 0.150 mol/L... 

Calculate the mass of silver metal that can be produced by the action of 12.2 g of cadmium metal on excess aqueous silver nitrate. 

Practice Problem 1 7.6 Calculate the mass of silver metal that will be deposited by passage of a 10.0-A current through a solution of silver nitrate for 3.00 h. I... 

A sample of a mixture containing only sodium chloride and potassium chloride has a mass of 4.000 g. When this sample is dissolved in water and excess silver nitrate is added, a white precipitate (silver chloride) forms. After filtration and drying, this precipitate has the mass 8.5904 g. Calculate the mass percent of each mixture component. 

You are given the mass of the reactant AgNOj and the actual yield of the product Ag2Cr04. You need to write the balanced chemical equation and calculate the theoretical yield by making these conversions grams of silver nitrate to moles of silver nitrate, moles of silver nitrate to moles of silver chromate, moles of silver chromate to grams of silver chromate. The percent yield can be calculated from the actual yield of product and the calculated theoretical yield. 

A mass of 1.50 g of silver is plated from a silver nitrate solution in 1.5 h. Calculate the (a) coulombs, (b) faradays, and (c) amperes necessary for this process. 

A button case for a small battery must be silver coated. The button is a perfect cylinder with a radius of 3.0 mm and a height of 2.0 mm. For simplicity, assume that the silver solution used for plating is silver nitrate. (Industrial processes often use other solutions.) Assume that the silver plating is perfectly uniform and is carried out for 3.0 min at a current of 1.5 A, (a) What mass of silver is plated on the part (b) How many atoms of silver have plated on the part (c) Calculate an estimate of the thickness (in atoms) of the silver coating. (Silver has a density of 10.49 g/cm and an atomic radius of 160 pm.)... 

Analysis Determine the mass of 2-chloro-2-methylbutane isolated and calculate the percent yield. Perform the alcoholic silver nitrate and sodium iodide/acetone classification tests on your product (Sec. 25.9). Obtain IR and NMR spectra of your starting material and product and compare them with those of authentic samples (Figs. 14.5-14.8). 

What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride Calculate the concentrations of each ion remaining in solution after precipitation is complete. 

A 450.0-mL sample of a 0.251-M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl in solution after the reaction is complete 116. The zinc in a 1.343-g sample of a foot powder was precipitated as ZuNH4P04. Strong heating of the precipitate yielded 0.4089 g Zu2P207. Calculate the mass percent of zinc in the sample of foot powder. 

Calculate the mass of silver bromide produced from 22.5 g of silver nitrate in the following reaction ... 

A student passed a constant electric current of 0.15 A through a solution of silver nitrate, using pure silver electrodes, for 45 min exactly. The mass of the anode decreased by 0.45 g. Use this data to calculate the charge on a mole of electrons. 

Is the anode reaction an oxidation or reduction reaction Explain your answer, c Explain why the silver nitrate solution becomes acidic during this electrolysis, d Calculate the mass of silver deposited at the cathode when the electrolysis is carried out for exactly 35 min using a current of 0.18A. (A [Ag] = 108 F=96500CmoH)... 

A 15.00-mL solution of potassium nitrate (KNO3) was diluted to 125.0 mL, and 25.00 mL of this solution were then diluted to 1.000 X 10 mL. The concentration of the final solution is 0.00383 M. Calculate the concentration of the original solution. When 2.50 g of a zinc strip were placed in a AgN03 solution, silver metal formed on the surface of the strip. After some time had passed, the strip was removed from the solution, dried, and weighed. If the mass of the strip was 3.37 g, calculate the mass of Ag and Zn metals present. 

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