An aqueous solution of nitric acid has a density of 1.084 g mL-1 and a measured concentration of 2.580 molar. What is the percent weight of nitric acid in the solution.

  1. 👍
  2. 👎
  3. 👁
  1. How much does a liter of solution weigh? It has a mass of 1.084 g/mL x 1000 mL = 1084 grams.
    There are 2.580 moles HNO3 in the 1084 g of solution; therefore, 2.580 x molar mass HNO3 = about 162 g HNO3. (You need to do it exactly).
    % HNO3 = (g HNO3/mass solution)*100 =
    about (162/1084)*100 = ??
    Check my work.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry(Urgent Please help)

    A student is asked to standardize a solution of barium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid). It requires 33.9 mL of barium hydroxide to reach the endpoint. A.

  2. Chemistry

    Students are instructed to add no more than 0.25 mL of 15 M nitric acid. What volume of 15 M nitric acid is required to react with 0.030 g of copper metal? If 1.0 mL of acid contains approximately 20 drops, how many drops of

  3. Chem Help!

    Assume that a given solution caontains Ag+or Ba2+ or a mixture of both. A reasonable method for doing a qualitative analysis on this solution might be sketched out as followes (remember || means a precipitate forms and | means a

  4. biology

    Nitric acid is a chemical that is used in the production of fertilizers. The chemical formula of nitric acid is HNO3. Which of the following are true for a nitric acid molecule? Select all that apply. It has three oxygen atoms. It

  1. Chemistry

    A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for

  2. chm

    An aqueous solution that is 10.0 percent sulfuric acid (H2SO4) by mass has a density of 1.143 g/mL. Determine the molality of the solution. ( 3 significant figures)

  3. chm

    An aqueous solution that is 30.0 percent sulfuric acid (H2SO4) by mass has a density of 1.105 g/mL. Determine the molarity of the solution.

  4. Chemistry 12

    9. According to Arrhenius, which of the following groups contain: i)only acids ii)only bases a. NaOH, H2CO3, KCl b. MgCl2, H2SO4, HCl c. HNO3, HCl, H3PO4 d. Mg(OH)2, AgBr, HF e. KOH, NH4OH, Ba(OH)2 10. Enough water is added to 100

  1. Chemistry-please help

    "Use a 10% w/v nitric acid solution." How to prepare 10% w/v nitric acid solution? Do I just weigh 10g of conc nitric acid (65%) and dilute to 100ml with water?

  2. chem

    On Easter Sunday, April 23, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate. 2 HNO3(aq) + Na2CO3(s) 2 NaNO3(aq) + H2O(l) + CO2(g) (a) Calculate H° for this

  3. chemistry

    Copper reacts with nitric acid according to the following reaction: 3 Cu (s) + 8 HNO3 (aq) --> 3 Cu(NO3)2 (aq) + 2 NO (g) + 4 H2O (l) If an pre 1982 copper penny contains 3.10 grams of copper, what volume of 8.00 M nitric acid is

  4. Chemistry

    Barium carbonate and nitric acid reacts in a double displacement reaction. One of products also dissociates and evolves carbon dioxide. Write the net ionic reaction including the proper use of phase labels for this solution run in

You can view more similar questions or ask a new question.