1. Questions

Chemistry

How much sulphuric acid containing 90% H2SO4 by wt. is needed for the production of 1000 kg of HCl containing 42% HCl by weight in this reaction.

2NaCl + H2SO4 -----> Na2SO4 + 2HCl

  1. 👍
  2. 👎
  3. 👁
Kritim

  1. mass HCl needed is 1000 kg x 0.42 = 420 kg or 420,000 g HCl, then mols HCl = 420,000/molar mass HCl = ?

    Using the coefficients in the balanced equation, convert mols HCl to mols H2SO4.
    Then grams H2SO4 (at 100%) = mols H2SO4 x molar mass H2SO4 = ?
    Since it is only 90% pure, you will need ?g H2SO4/0.90 = ?

    1. 👍
    2. 👎
    DrBob222

  2. 626.484kg

    1. 👍
    2. 👎
    Binayak

  4. How did you got the answer show full steps!!

    1. 👍
    2. 👎
    Sanjog

  5. No proper answer. Actual answer is 628kg

    1. 👍
    2. 👎
    Pooja

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A commercially available sample of sulphuric acid is 15% H2SO4 by mass (density=1.10g/ml) Calculate the molarity ,normality and molality.

  2. pcc

    A volume of 40.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 21.7mL of 1.50 M H2SO4 was needed? The equation is

  3. Chemistry

    Automobile batteries use 3.0 M H2SO4 as an electrolyte. How much 1.20 M NaOH will be needed to neutralize 225mL of battery acid?

  4. Chemistry

    A volume of 70.0mL of aqueous potassium hydroxide(KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the solution if 19.2mL of 1.50M H2SO4 was needed? The equation is

  1. Chemistry

    Sulfuric acid is commonly used as an electrolyte in car batteries. Suppose you spill some on your garage floor. Before cleaning it up, you wisely decide to neutralize it with sodium bicarbonate (baking soda) from your kitchen. The

  2. Chemistry

    Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in

  3. science

    Concentrated sulfuric acid (18.4 molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead

  4. chemistry

    Consider the following reaction: 3 C2H5OH + 2 K2Cr2O7 + 8 H2SO4 → 2 Cr2(SO4)3 + 3 CH3COOH + 2 K2SO4 + 11 H2O Which statement below best describes what is happening as this reaction proceeds? a. sulphuric acid is being reduced to

  1. chemistry

    3-pentanol is heated with sulphuric acid (H2SO4) to become compound M. Compound M is reacted with Br2/ H2O to form Compound N. Outline the reaction step and name the compound M and N

  2. chemistry

    The reaction SO2 + H2O =H2SO4 Is the last step in the commercial production of sulfuric acid . the enthalpy change for this reaction is -227 KJ . In designing a sulfuric acid plant is it necessary to provide for heating or cooling

  3. Chemistry

    Ca3(PO4)2 + 3 H2SO4 -> 3 CaSO4 + 2 H3PO4 What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?

  4. Science

    How do I prepare 1% H2SO4 from concentrated sulphuric acid (96% with density 1.84g/ml)? Thank you very much for your help.

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