A 50.00-mL solution containing NaBr was treated with excess AgNO3 toprecipitate 0.214 6 g of AgBr (FM 187.772). (a) How many moles of AgBr product were isolated? (b) What was the molarity of NaBr in the solution?

(ii) H3CO H 1. excess CH3OH, [H+] 2. LDA, THF 3. H3C- 4. LiAlH4 5. H* workup 6. H3O+ e

K2CO3(aq) + 2HC2H3O2(aq) yields  2KC2H3O2(aq) + H2O(l) + CO2(g) How many moles of H2O can be obtained from 25.0 ml of 0.150 M HC2H3O2?

Z question conc... → Q1/ A solution was prepared dissolving 329 mg of K,Fe(CN), in sufficient water to give 750 ml. calculate (a) the molar concentration of K. (b) The mass/volume percentage of K,Fe(CN),. mber of millimoles of K in 50.0 mL of this solution. (d) the concentration of [Fe(CN).J* in ppm. K=39 Fe=56 C=12 N=14 Q2/ calculate the p-value for each ions in the following solutions (a) 0.02 F BaCl,.2H,0 ? (b)25 ml of 0.04 M HCI mixed with 50 ml of 0.02 M NaOH

What is the water solubility of BaCO3 (Kep = 2.6 x 10-9) in a solution containing 0.40 M CO, (aq)? %3D

The Kjeldahl method was used to determine the nitrogen content of a protein. A 275 µL aliquot of a 47.0 mg/mL protein solution was digested in boiling sulfuric acid. The solution was made basic and the liberated NH, was collected in 5.00 mL of 0.0512 M HCl. A volume of 7.00 mL of 0.0174 M NaOH was required to react with the excess HCl. Calculate the weight percent of nitrogen in the protein. weight percent: wt% N

A sample of alfalfa meal weighing 2.0 g is analyzed by Kjeldahl method for the percentage of nitrogen. The liberated NH3 is caught in a solution of H3BO3, and 8.23 ml of HCl are required in the subsequent titration. A sample of pure (NH4)2SO4 (132.12) weighing 0.61 g is treated with excess NaOH and the liberated NH3 (17.04) is also caught in H3BO3. The resulting solution requires 20 ml of the acid for titration. Calculate the percentage of protein in the sample using 6.25 as the factor.

6. (2 pts) Aqueous solutions of a compound did not form precipitates with Cl', Br', I, SO,²', CO;²', PO4³-, OH", or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified with HCl (aq). This compound is A) Pb(NO3)2 B) (NH4)2S C) KBr D) Li2CO3 E) AgNO3

7:36 .l LTE Unanswered •1 attempt left • Due on Oct 6, 7:00 PM What is the sulfate ion concentration of the resulting solution when 75.0 mL of 1.50 M CUSO4 and 50.0 mL of 1.00 M Co2(S04)3 are mixed together? А 4.50 M B 2.50 M C 2.10 M D 1.30 M 1.25 M Submit