Include an annotated calculation showing how you determined the Kai and Ka2 (i.e. How did you find Ka1 and Ka2?). Provide a percent error comparing your experimental molar mass to the accepted value. 1. Determining the Molar Mass of the Acid • Given mass of acid: 0.120 g • Volume of NaOH solution at first • equivalence point: 12.5 mL Molarity of NaOH: 0.1 M Calculation of moles of NaOH: [ \text{Moles of NaOH} = \text{Molarity} \times \text{Volume} = 0.1, M \times 0.0125, L = 1.25 \times 10^{-3}, \text{mol} ] Moles of Acid: Since the acid is diprotic, the moles of acid will be half the moles of NaOH used: [ \text{Moles of Acid} = \frac{1.25 \times 10^{-3}, \text{mol}}{2} = 6.25 \times 10^{-4}, \text{mol} ] Molar Mass of the Acid: [ \text{Molar Mass} \frac{\text{Mass of Acid}} = {\text{Moles of Acid}} = \frac{0.120, \text{g}}{6.25 \times 10^{-4}, \text{mol}} = 192, \text{g/mol} ] 2. Determining (K_a1) and (K_a2) • ⚫ pH at the first half-equivalence point (pH 1st half): 2.91 ⚫ pH at the second half-equivalence point (pH 2nd half): 7.5 Since pKa = pH at half equivalence point: (K_{a1}): [pka_1 = 2.91 ] [ K_{a1} = 10^{-2.91} \approx 1.23 \times 10^{-3}] (K_{a2}): [ pKa_2 = 7.5 ] [ K_{a2} = = 10^{-7.5} \approx 3.16 \times 10^{-8} ]

In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)

A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?

In a 4.9 mm aqueous solution of benzoic acid (C6H₂CO₂H), what is the percentage of benzoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. O Round your answer to 2 significant digits. []% x10 X Ś |||

I gave the wrong molarity when I submitted this last. I used 25 ml of HCl. The molarity of NaOH is 0.1065 instead of what I have in the image. Sorry again,but thank you!

. Calculate the moles of H+ delivered to eachsample based on your experimental dataand record these values in Data Table 2.  0.1M HCl = 0.1 moles HCl / 1 Liter solutionCalculate the moles of OH- in each sampleand record these values in Data Table 2. H+ + OH- H2O Calculate the moles of Ca2+ in each sampleand record these values in Data Table 2. Ca(OH)2 Ca2+ + 2OH24. Calculate the molar solubility of Ca(OH)2for each sample and record these values inData Table 1. Molar solubility = moles / Liter       Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 25.37 25.37 25.37 Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 28.18 28.21 28.28 Mass of Calcium Hydroxide Solution       Volume of Ca(OH)2 Density = 1.000 g/mL       Concentration of HCl (M)       Initial HCl volume in Syringe 1.0ml 1.0ml 1.0ml Final HCl volume in Syringe .54ml .58ml .5ml Volume of HCl Delivered .46ml .42ml…

I dont know how to do this question

Given chart information attached Calculate the number of moles of acid

It requires 10.75 mL of 1.05 M Ba(OH)2 to neutralize (titrate) a 35.00 mL sample of HX. What is the concentration of HX solution (measured in moles per liter)? Report to 3 significant figures.

Constants | Periodic Table These questions refer to determing unknown concentrations of acids and/or bases. Part A In a titration experiment, a solution of rubidium hydroxide (RBOH) of unknown concentration was titrated with a solution of nitric acid (HNO3) of known concentration. 15.00 mL of the unknown rubidium hydroxide (RbOH) solution required 23.21 mL of 0.1429 mol L-1 nitric acid (HNO3) solution. What is the concentration of the rubidium hydroxide (RbOH) solution? OH 9.235x10-2 mol L-1 0.2211 mol L-1 0.2322 mol L- 0.1429 mol L-1 0.2587 mol L |-1