chemistry

X is a solution,of dibasic of H2X. G is a solution containing 1.00g of NaOH in 250cm3 of solution . 24.60cm3 of solution F required 25.00cm3 of solution G . From your result and information provided above. (I)concentration of G in mol/dm3 (ii) concentration of F in mol/dm3 (iii) molar mass. Of acid H2X given that 100cm3 of solution F contained 0.495g of acid (H-1.00,O-6,Na-23)

  1. 👍 0
  2. 👎 0
  3. 👁 122
  1. You made a typo. O is 16 not 6.
    i) concn G is 0.1 mol/dm3. Calculated as follows:
    mols NaOH = g/molar mass = 0.1/40 = 0.025
    M NaOH = 0.025/0.25 = 0.1 mol/dm3

    ii)Note: 1 L = 1 dm3 and M = mols/dm3
    2NaOH + H2X ==> Na2X + 2H2O
    mols NaOH used = M x L = 0.1M x 0.025 = 0.0025
    mols H2X (F) = 1/2 x 0.0025 = 0.00125
    M F = mols/L = 0.00125/0.0246 = 0.051M = 0.051 mol/dm3 but you may want the answer more accurate than that.

    iii)
    mols H2X in 100 cc = M x L = 0.051 x 0.1 = 0.0051
    mols = grams/molar mass or
    molar mass = grams/mols = 0.495/0.00508 = ?

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. College Chemistry

    I need help with this question!! a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of

    asked by Emily on April 25, 2012
  2. Chemistry

    A 0.1873 g sample of a pure, solid acid, H2X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is H2X(aq) + 2NaOH(aq) ¨ Na2X(aq) + 2H2O(l) If the

    asked by Lauren on May 11, 2011
  3. Chemistry

    Question: A solution of H2X of unknown concentration is given. pH of the solution is 4. ka1=2*(10)^-6 M ka2=1*(10)^-11 M Find the concentrations of [H2X] ,[HX-] and X^2- in the solution. My thoughts on the question: The

    asked by Shenaya on May 31, 2017
  4. Chemistry

    Question : ka1 and ka2 values of H2X is given 1*(10)^-5 M and 1*(10)^-9 M.50cm^3 of 0.2 M KOH and 50 cm^3 of H2X of unknown concentration is mixed together and the pH of the final solution is given as 7. 1)Find the concentration

    asked by Aanya on May 20, 2017
  5. chemistry

    Question : ka1 and ka2 values of H2X is given 1*(10)^-5 M and 1*(10)^-9 M.50cm^3 of 0.2 M KOH and 50 cm^3 of H2X of unknown concentration is mixed together and the pH of the final solution is given as 7. 1)Find the concentration

    asked by To Aanya on May 21, 2017
  6. chemistry

    Calculate the volume of concentrated NaOH solution (which contains 500.00g of NaOH per liter of solution) that you will need to make 1.00L of a 0.100M NaOH solution

    asked by xx on October 28, 2014
  7. Chem: pH of acids and bases

    Calculate the concentrations of all species in a 0.320-M solution of H2X if K1 = 6.31E-06 and K2 = 3.71E-09 [H2X] = [H3O1+] = [HX1-] = [X2-] = Work: H2X + H2O --> HX- + H3O+ .320 M This is literally the only thing I know. How can

    asked by Maggie on October 24, 2016
  8. Chemistry

    So this is a three part question. I solved the first part correctly but I need help with the second and third. Q: The dissociation equilibrium constants for the protonated form of of alanine (a diprotic amino acid, H2X+)are Ka1 =

    asked by Maria on May 9, 2017
  9. chemistry

    1.25 grams of an acidnis completely neutralised by 25ml of a 0.25M Ba(OH)2 SOLUTION.which of the following statements are correct. a)if the acid is dibasic its molar mass would be 200 b)if it is dibasic /0.5g of the acid would

    asked by akshita on September 27, 2017
  10. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH

    asked by djella on October 25, 2011

More Similar Questions