chemistry

I need some help with calculating percent yield and percent purity of aspirin.

Here's my data (questions follow):

SYNTHESIS
Mass of salicylic acid.., 2.0 g
Volume of acetic anhydride.., 5 mL
Mass of watch glass.., 22.10 g
Mass of aspirin and watch glass.., 28.01 g
Mass of aspirin.., 5.91 g

DETERMINATION OF PURITY
Mass of aspirin.., 0.34 g
Concentration of NaOH.., 0.1 M
Initial buret reading.., 0 mL
Final buret reading.., 15.8 mL
Volume of NaOH used.., 15.8 mL
Number of moles of NaOH required.., 1.60 x10^-3 mol

1. Calculate your mass percent yield of aspirin.

(actual yield, g/theoretical yield, g) x 100

Not sure what numbers I'd use here...

2. Calculate the percent purity of your aspirin.

(mass of aspirin, g (titration)/mass of aspirin, g (synthesis)) x 100

(0.34 g/5.91 g) x 100 = 5.8%

I'm pretty sure that's right, but not completely.


patience. Answered below on the original post.

  1. 👍 0
  2. 👎 0
  3. 👁 242
  1. I need help with this What mass of bleach (NaCLO; 74.44g/mol) could be made from 72.0 g of NaOH and 72.0 g Cl2 at 95.0 % yield

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Finance

    A 7.10 percent coupon bond with 14 years left to maturity is priced to offer a yield to maturity of 7.9 percent. You believe that in one year, the yield to maturity will be 7.4 percent. What is the change in price the bond will

    asked by BB on July 4, 2020
  2. FINANCE

    Yield to call Six years ago, the Singleton Company issued 20-year bonds with a 14 percent annual coupon rate at their $1,000 par value. The bonds had a 9 percent call premium, with 5 years of call protection. Today, Singleton

    asked by Mel on September 18, 2007
  3. alg 1

    Find the percent error in calculating the volume of the prism. V=(bw)(h) v=11 x 8 (7) V=616 my choices were: 19% 10% 119% 83% I'm not sure what it means to find the percent error. Please explain. Thanks.

    asked by Jane on April 16, 2013
  4. Chemistry

    Consider the following reaction: 2 SO2 (g) + O2 (g)----> 2 SO3 (g) If 285.3 mL of SO2 is allowed to react with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and theoretical yield of SO3 in

    asked by Jarrod on October 27, 2010
  5. DESPERATE NEED OF HELP--Chemistry, almost done

    Calculating Yield--need some help finishing problem. Almost done, just need help one ONE step, please help!!? Well we did a lab on limiting reagent/reactants. The balanced equation is Sr(NO3)2 + 2KIO3 --> Sr(IO3)2 + 2KNO3 Mols of

    asked by Angie on February 28, 2007
  1. chemistry

    1. Chlorobenzene, C6H5Cl, is used in the production of chemicals such as aspirin and dyes. One way that chlorobenzene is prepared is by reacting benzene, C6H6, with chlorine gas according to the following BALANCED equation. C6H6

    asked by Michael on March 31, 2010
  2. chemistry

    A student prepared aspirin (C9H8O4) in a laboratory experiment using the following reaction. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 The student reacted 2.00 g salicylic acid (C7H6O3) with 2.67 g acetic anhydride (C4H6O3). The yield was

    asked by lyne on February 4, 2009
  3. Chemistry

    Aspirin is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H603. The other product produced is acetic acid, C2H402. C7H6O3+C4H6)3->C9H8O4+C2H4O2 What is the theoretical yield in grams of aspirin, C9H8O4, when

    asked by Lauren on November 6, 2012
  4. chemistry - synthesis of aspirin

    wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid? If so, how do we find the mass of acetic acid in this experiment volume of acetic

    asked by Priscilla on April 7, 2012
  5. chemistry

    a student synthesized 6.895g of barium iodate monohydrate, Ba(IO3)2.H2O, by adding 30.00 mL of 5.912*10^-1M barium nitrate, Ba(NO3), to 50.00 mL of 9,004*10^-1 M sodium iodate, NaIO3 (1) write the chemical equation for the

    asked by aymal on March 1, 2010
  6. Math

    Go to Table 10-1 which is based on bonds paying 10 percent interest for 20 years. Assume interest rates in the market (yield to maturity) decline from 11 percent to 8 percent: A. What is the bond price at 11%? B. What is the bond

    asked by Robert on January 11, 2010

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