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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 solution. What is the molarity of the NaOH solution?

3. a 0.481 gram sample of an unknown acid (HX) required 28.95 mL of 0.2103 M NaOH for neutralization to a phenolphthalein endpoit. What is the molar mass of the acid?

4. what volume of 0.1037 M HCL is necessary to neutralize 0.3643 grams Ca(OH)2? included a balanced equation?

5.calculate the molar concentration of propionic acid (HC3H5O2) in solution if 10.00mL of a propionic acid solution is neutralized with 16.85mL of 0.143 M NaOH solution.

6. calculate the mass percent of propionic acid (HC3H5O2) in solution. (Assume the density of the solution to be 1.00g/mL.)

  • chemistry - ,

    You fare better if you post one question per try.
    M1 x mL1 = M2 x mL2

    Since NaOH and HCl react 1:1 (write the balanced equation to see that), then
    mLHCl x MHCl = mLNaOH x M NaOH

    moles NaOH = M x L = ?
    moles HX = the same
    moles HX = grams/molar mass
    Solve for molar mass.

  • chemistry - ,


  • chemistry - ,

    which of the following Al acid ?(1)s2- (ii)H3O+ (iii)NO3- (iv)k+

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