chemistry

determine the quantity of NaOh whose percentage is 15 % to balance 176 g of H2SO4

  1. 👍 0
  2. 👎 0
  3. 👁 120
  1. Do mean to calculate the volume of NaOH required for the neutralization?
    2NaOH + H2SO4 ==> Na2SO4 + 2H2O

    moles H2SO4 = grams/molar mass
    Use the coefficients in the balanced equation to convert moles H2SO4 to moles NaOH.
    15% NaOH means 15 g/100 mL (is that 15% w/v?)
    So 15 g NaOH = ?? moles.
    moles/0.1 L = M
    Then M NaOH = moles NaOH/L NaOH
    Substitute MNaOH, moles from above of NaOH needed, solve for L NaOH needed.
    Post your work if you get stuck.

    1. 👍 0
    2. 👎 0
  2. i need to calculate the mass (m ) of NaoH with C% = 15 % , to balance 176 g of H2SO4

    so i though to use this method
    C% = mass of h2s04 / mass of h2so4 + mass of Naoh which is unknown

    mass of Naoh = c% x mass of h2so4 / 100

    is this the right method or not ?

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    You place a piece of paper on a balance and find that its mass is 0.63 g. You add a lump of NaOH to the paper and get a mass of 22.21 g. You remember that you forgot to tare the balance before taking this measurement. You tare the

  2. chemistry (Pls Bob check for me)

    A 0.5g of fuming h2so4 oleum is diluted with water. This solution is completedly neutralized by 26.7ml of 0.4N naoh. Find the percentage of free so3 in the sample The asnwer 20.6% My calculation h2so4= 98/2 = 49 so3= 80/2 = 40

  3. chemistry

    A 25.0-mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of 0.150 M NaOH are required to completely neutralize the acid?

  4. Chemistry

    One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concentration of NaOH is normally in the range of 3 to 6 M. The NaOH is

  1. Biology

    You place a piece of paper on a balance and find that its mass is 0.63 g. You add a lump of NaOH to the paper and get a mass of 22.21 g. You remember that you forgot to tare the balance before taking this measurement. You tare the

  2. chemistry

    When 25.0 mL of 1.0 M H2SO4 is added to 50.0 mL of 1.0 M NaOH at 25.0 °C in a calorimeter, the temperature of the aqueous solution increases to 33.9 °C. Assuming the specific heat of the solution is 4.18 J/(g·°C), that its

  3. Chemistry

    P4O10(s) + 6 H2SO4(l) --> 4 H3PO4(aq) + 6 SO3(g) Pure H2SO4(l) has a density of 1.84 g/mL. If 45.0 mL of H2SO4(l) reacts: What mass of P4O10 reacts? - it's given 45.0 mL of H2SO4 with the density of 1.84 g/mL, so the mass of H2SO4

  4. Chemisty

    A 25-mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4. What is the molarity of the sulfuric acid solution? A. 0.004M H2SO4 B. 0.235M H2SO4 C. 0.117M H2SO4 D. 0.002M H2SO4

  1. College-Chemistry

    NaOH(s)+ H2SO4(aq)=Na2SO4(aq) + H2O(l) Consider the unbalanced equation above.A 0.900 g sample of impure NaOH was dissolved in water and required 37.0 mL of 0.145 M H2SO4 solution to react with the NaOH in the sample. What was the

  2. Chemistry help

    NaOH+H2SO4-> H2o+Na2SO4? How many moles of NaOH required to neutralize 1 mole H2SO4?

  3. chemistry

    qualitative organic analysis lab 1. Why is it important to have clean test tubes before running a test? Before which tests should acetone not be used to clean the test tubes? 2. Why run solubility tests before running the

  4. CHEMISTRY

    25cm^3 of a solution of NaOH required 28cm^3 of 1.0 mol dm^-3 H2SO4 to neutralise it. a)Write an equation for the reaction. b)How many moles of H2SO4 were needed? c)How many moles of NaOH were thus neutralised? d)How many moles of

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