chemistry

What will be the pH of hydrochloric acid after 0.01M of hydrochloric acid is diluted by the addition of 80ml distilled water?

  1. 👍 0
  2. 👎 0
  3. 👁 213
  1. Depends upon how much 0.01 M was diluted. You should proof your posts.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem

    The mass of a beaker is 5.333g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. From the data, what is the

  2. Chemistry

    Q1. A 0.5 g mixture of Cu2O and CuO contain 0.425 g Cu. What is the mass of CuO in the mixture? Q2. A chemist wants to prepare 0.5 M HCl. The label of a commercial hydrochloric acid shows that S.G. =1.18 and concentration of HCl

  3. Chemistry Please help

    A bottle of 12.0 M hydrochloric acid has only 35.7 mL left in it. What will the HCl concentration be if the solution is diluted to 250.0 mL?

  4. College Algebra

    How many liters of 80% hydrochloric acid must be mixed with 40% hydrochloric acid to get 15 liters of 65% hydrochloric acid? Write your answer rounded to three decimals. Show all work.

  1. chem

    What mass of hydrochloric acid (in grams) can be neutralized by 2.3g of sodium bicarbonate? (: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)

  2. Chemistry

    Which of the following aqueous solutions are good buffer systems ? . 0.26 M hydrochloric acid + 0.24 M potassium chloride . 0.14 M acetic acid + 0.20 M potassium acetate . 0.16 M potassium hypochlorite + 0.23 M hypochlorous acid .

  3. Science

    G) The mass of a beaker is 40.94 g. After 5.00 mL of concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and hydrochloric acid is 46.92 g. From the data, calculate the density of

  4. Chem

    The mass of a beaker is 5.333g. After 5.00 mL of a concentrated hydrochloric acid solution is pipetted into the beaker, the combined mass of the beaker and the hydrochloric acid sample is 11.229 g. From the data, what is the

  1. Chemistry

    The reaction of hydrochloric acid (HCl) with ammonia (NH3) is described by the equation: HCl + NH3 → NH4Cl A student is titrating 50 mL of 0.32 M NH3 with 0.5 M HCl. How much hydrochloric acid must be added to react completely

  2. chem

    Which of the following could be added to a solution of sodium acetate to produce a buffer? ? A) acetic acid only B) acetic acid or hydrochloric acid C) potassium acetate only D) sodium chloride or potassium acetate E) hydrochloric

  3. chemistry

    An aqueous solution is 40.0% by mass hydrochloric acid, HCl, and has a density of 1.20 g/mL. The molality of hydrochloric acid in the solution is m.

  4. Chemistry

    The density of a solution of hydrochloric acid is 1.0929 g/cc, and it is 19.00 percent by mass. What volume of the solution (in milliliters) do you need to supply 30.0 g of hydrochloric acid? I'm not sure how to start

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