A 0.3202 (±0.0001) g sample of a pure monoprotic acid required 20.04 (+0.02) cm of 0.1005 (+0.0005) mol dm -1 neutralisation. Find the molar mass of the acid in g mol together with its uncertainty also in g mol, NAOH for ', with an appropriate number of digits. Select one: 1.59 x 102+ 0.2 g mol -1 b. 1.60 x 10 + 0.03 g mol C. 1.590 x 10 +0.03 g mol d. 590 x 102 ±0.2 g mol 1.60 x 102+ +0.2 g mol1 e. Clear my choice

\table [Index Code,Statistic Date,Instrument Dividend Yield], [J100, 2019/01/31, Accentuate,8,08% T Index Code Statistic Date Instrument Dividend Yield J100 2019/01/31 Accentuate 8,08% J100 2019/02/28 Accentuate 7,22% J100 2019/03/31 Accentuate 6,22% J100 2019/04/30 Accentuate 9,95% J100 2019/05/30 Accentuate 8,85% J100 2019/06/30 Accentuate 9,98% J100 2019/07/31 Accentuate 9,31% J100 2019/08/29 Accentuate 3,18% J100 2019/09/30 Accentuate 5,14% 100 2019/10/31 Accentuate 10,15% J100 2019/11/28 Accentuate 8,89% J100 2019/12/31 Accentuate 10,99% 4.1 Using dividend yield as returns. Consider an investor with a portfolio consisting only of Accentuate shares. Calculate the Treynor ratio given that the beta of Accentuate is 0.8 (8 marks) 4.2 Consider an investor with a portfolio consisting only of Accentuate shares Given that the J100 market index was 5%. Calculate the Jensen alpha given that Accentuate beta is 0.8 (8 marks) 4.3 Calculate the expected return of a portfolio consisting of 40%…

If pH (± 0.5 pH units) strips were used to determine the equivalence point at pH=8.5. What is the relative error (%) in pH at the equivalence point? I assumed it should be 0.5/8.5 * 100 = 5.88, rounded to 5.9 for sig figs. but I got the answer wrong. Please help and let me know how to solve this.

Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a %3D standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). %3D Formula Masses: AgNO3 = 169.87; CI = 35.45 Calculate the following: 1. Molar concentration of KSCN solution M %3D 2. Molar concentration of AgNO3 solution M %3D 3. % (w/w) chloride in the original sample =

Suppose that you used smaller volumetric apparatus to prepare 0.250 M NH3 solution by diluting 84.6 (±0.8) µL of 28.0 (±0.5) wt% NH3 up to 5.00 (±0.02) mL. Find the uncertainty in 0.250 M.

Suppose a 0.048 M aqueous solution of sulfuric acid (H₂SO₂) is prepared. Calculate the equilibrium molarity of SO of sulfuric acid in the ALEKS Data resource. Round your answer to 2 significant digits. DM 0.2 X ? Help You'll find information on the properties

3. If AH*= 10 kcal/mol and AS = +10 eu, at what temperature will AG = 0? Show your work. %3D

Please help.

Make sure the answer has correct significant di

Given: Trial 1 25.00 0.00 10.40 10.40 Trial 2 25.0 10.40 20.13 9.73 Volume of Ca(OH)2 (mL) Initial burette reading (mL) Final burette reading (mL) Volume of HCl used in titration (mL) answer in 3 significant figures. Trial 3 25.0 20.13 30.29 (a) write the neutralization reaction involved in the experiment. (b) Calculate the molarity of Ca2+ (M). Show the complete solution. 10.16