A 250 mL flask contains a 8.0% (m/v) nitric acid solution. Which TWO of the following...
17. The density of nitric acid (which is HNO3 in water) is 1.42 g/mL. The m/m% of HNO, in nitric acid is 69% m/m. How many grams of HNO3 are in 1 mL of nitric acid? a) 0.99g b) 99g c) 2.1g d) 0.021 g e) 0.49g
71. A solution of nitric acid has a density of 1.5 g/mL and is 20% by weight HNO3. a. What is the molarity of this solution of HNO;? b. What volume of this solution should be taken in order to prepare of 5.0 L of a solution of 0.15 M nitric acid by dilution with water? In order to obtain a precise concentration, the 0.15 M HNO solution is standardized against pure Hgo (molar mass = 216.59 g/mol) by titrating...
A 20.00 mL, sample of 0.1015 M nitric acid is introduced into a flask, and water is added until the volume of the solution reaches 250. mL. What is the concentration of nitric acid in the final solution? 1.27 M 5.08 times 10^-4 M 8.12 times 10^-3 M 0.406 M 3.25 times 10^-2 M A buret is read to how many decimal places? can only be read to the ones place so no decimal places 1 2 4 3
A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0%HNO; by mass. What mass of HNO3 is present per liter of solution?
21. Commercial grade fuming nitric acid contains about 90% HNO3 by mass with a density of 1. 50 g/mL, calculate the molarity of the HNO, solution. A. 0.214 M B. 21.4M c. 2.14 M
) Calculate the volume (in mL) of nitric acid that you plan to use in Reaction 1 in the procedure. Cu(s) + 4HNO3(aq) -----> Cu(NO3)2 (aq) + 2NO2(g) + 2H2O (l) 2) Calculate the amount of zinc granules (in grams) that must be added in reaction 5 in part 1 of the procedure CuSO4 (aq) + Zn (s) ------> ZnSO4 (aq) + Cu (s) Additional Information from procedure 1) . Weigh out approximately 0.50 g (starting material) of copper wire...
Analysis of Vinegar EXPERIMENT NAME SECTION DATE POSTLABORATORY ASSIGNMENT 1. A standard nitric acid solution is prepared using 0.425 g of sodium carbonate, NaCO3. Find the molarity of the acid if 33.25 mL are required to reach a permanent endpoint. 2 HNO, (aq) + Na2CO3(s) + 2 NaNO3(aq) + H2O(l) + CO2(g) 2 H OT 2. A 10.0-ml sample of household ammonia solution required 27.50 mL of 0.241 M HNO3 for neutralization. Calculate (a) the molar concentration of the ammonia...
B. Commercial nitric acid comes in a concentration of 16.0 mol/L. The density of this solution is 1.42 g/mL Calculate the percent (w/w) of nitric acid, HNO3, in this solution. How many milliliters of the concentrated acid have to be taken to prepared 250 g of a solution that is 10.0%(w/w) HNO3? C. Citric acid, H3C6H5O7, occurs in plants. Lemons contain 5% to 8% citric acid by mass. The acid is added to beverages and candy. An aqueous solution...
36) 1. An aqueous solution contains 0.219 M carbonic acid and 0.166 M nitric acid. Calculate the carbonate ion concentration in this solution. [CO32-] = ____mol/L. 2. An aqueous solution contains 0.110 M carbonic acid and 0.146 M perchloric acid. Calculate the carbonate ion concentration in this solution. [CO32-] = _____mol/L.
Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iron Fe(NO3)3 2.50 x 10 in 0.10 M HNO3 nitric acid HNO3 0.10 120 35 50 250 conc. SCN KSCN 0.50 30 50 dilute SCN KSCN 2.50 x 10-3 30 50 Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5...