Calculate the pH of a 0.200M solution of zinc nitrate, Zn(NO₃)₂.
A chemist prepares a solution of zinc nitrate (Zn(NO)) by measuring out 14.4 g of zinc nitrate into a 500 ml. volumetric flask and filling the flask to the mark with water Calculate the concentration in mol/L of the chemist's zinc nitrate solution. Round your answer to 3 significant digits.
A chemist prepares a solution of zinc nitrate Zn NO 3 2 by measuring out 2.5x 10^2 μmol of zinc nitrate into a 300. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's zinc nitrate solution. Round your answer to 2 significant digits.
The chemical formula for zinc nitrate is: Zn(NO3)2 Calculate the molar mass of zinc nitrate. Round your answer to 1 decimal place. x10 g - mol
A chemist adds 415.0 mL of a 1.4M zinc nitrate (Zn(NO). solution to a reaction flask. Calculate the mass in kilograms of zinc nitrate the chemist has added to the flask. Round your answer to 2 significant digits. 5 ?
O STOICHIOMETRY Dilution A chemist makes 570 mL of zinc nitrate (Zn(NO3), ) working solution by adding distilled water to 190 ml of a 0.0381 M stock solution of zinc nitrate in water. Calculate the concentration of the chemist's working solution. Be sure your answer has the correct number of significant digits. X 5 ?
Nitric acid and zinc react to form zinc nitrate, ammonium nitrate, and water. 4 Zn(s) + 10 HNO3(aq) - 4 Zn(NO3)2(aq) + NH4NO3(aq)+ 3 H20(0) (a) How many atoms of zinc react with 1.05 g HNO3? atoms (b) Calculate the number of grams of zinc that must react with an excess of HNO3 to form 28.3g NH4NO3
A 20.0mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: a. 15.0mL b. 35.0mL
When a clean Manganese piece is placed in an aqueous solution of zinc nitrate, the piece becomes coated with a silver material. What is the material coating the manganese? [ Select ] ["zinc", "manganese", "zinc nitrate", "manganese(II) nitrate", "nitrate ions"] What are the oxidizing and reducing agents? Oxidizing agent [ Select ] ...
Consider a 100mL buffer solution prepared to be 0.200M HC2H302 and 0.200M KC2H302. Calculate the pH of the buffer system after 0.0040 mol of NaOH are added. A. 4.569 B. 4.921 C. 7.00 D. 11.602 The correct answer is B, but I need to show my work which I am not sure how to do.
Two liters of a standard Zn^2+ solution is to be made by dissolving 0.5265g solid zinc nitrate hexahydrade in 100mL of 0.100 MHNO_3. The solution was made up to two liters in volume. What is the concentration of the Zn (ppm) standard solution?