er Write the mass balance for a K2CO3 solution if the species in the solution are K+, CO32-, HCO3, H2CO3, H+, and OH¯. [K]+[H+] = [CO2]+[HCO3] + [H2CO3] + [OH-] [K] = 2[CO2] + [HCO3 ] + [H2CO3] [K+] = 2([CO32] + [HCO3 ] + [H2CO3]) [K] + [H+] = 2[CO32 ] + [HCO3] + [OH-] 2[K] = [CO32] + [HCO3 ] + [H2CO3]

er Write the mass balance for a K2CO3 solution if the species in the solution are K+, CO32-, HCO3, H2CO3, H+, and OH¯. [K]+[H+] = [CO2]+[HCO3] + [H2CO3] + [OH-] [K] = 2[CO2] + [HCO3 ] + [H2CO3] [K+] = 2([CO32] + [HCO3 ] + [H2CO3]) [K] + [H+] = 2[CO32 ] + [HCO3] + [OH-] 2[K] = [CO32] + [HCO3 ] + [H2CO3]

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 6P

See similar textbooks

Similar questions

Write a mass balance for a solution of Fe2(SO4)3 if the species are Fe3, Fe(OH)2, Fe(OH)2, FeSO4, SO24, and HSO4.
How to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.
A. Calculate the final percent concentration of the erythrocytes in each well: (NaCl, CaCl2, MgCl2) each solution has a concentration of 0.25M erythrocyte suspension solution (1mL of erythrocyte solution containing 10% washed red blood cells.) 135 microliters of each solution were added to individual wells + 15uL of the erythrocyte solution ex: Well #1= 135uL of (0.25M CaCl2 + 15uL erythrocyte sol.) B. What would be the final concentration of a well with 135uL (0.125M NaCl) + 15 uL erythrocyte solution?
A chemist attempts to prepare some very pure crystals of borax by dissolving 100g of Na 2 B 4 O 7 in200 grams of boiling water. He then cools the solution slowly until some borax crystallizes out.Calculate the grams of borax recovered in the crystals per 100 grams of initial solution (Na 2 B 4 O 7plus water), if the residual solution at 55 0 C after the crystals are removed contains 12.4%Na 2 B 4 O 7 . What is the percent yield or percent recovery of Na 2 B 4 O 7 . (MW: Na =23, O =16, B=10.8,H =1) round off up to 4 decimal places
Prepare the following solutions: 100.0 mL 0.0500 M stock Ca2+ solution 50.0 mL 0.0050 M working standard Ca2+ solution from 0.0500 M Ca2+
Assume you dissolve 30.0 g of cobalt sulfate heptahydrate (CoSO4.7H2O) in 500 ml of a 1.0 MH2SO4 solution. Calculate the following for CoSO4.7H2O in this solution:(The Specific Gravity of 1.0 M H2SO4 @ 20°C is 1.0814 g/ml.) Molality, Mole fraction and Weight percentage
The molar conductivities at infinite dilution of aqueous solutions of NH4Cl, NaCl, and NaOH are, respectively, 130, 108.6, and 216.5 S cm2 mol-1 at 18°C. The specific conductivity of a 0.01 M solution of ammonia at the same temperature is 9.6 x 10-5 [S cm-1] and the ion product of water is 0.59 x 1014. Determine: • The concentration of NH4+ ions in the ammonia solution. • The pH of the ammonia solution.
a 10g soil sample was gently stirred with 250 ml of 1.0 M CH3COO(NH4) solution for 24 h and centrifuged to separate the solution. The solution recovered after centrifugation was titrated with distilled water to a volume of 1 liter and analyzed for cations. Analytical results showed that the solution contained 20 mg/L Ca, 2 mg/L Mg, 1 mg/L K, and 0.5 mg/L Na. Calculate the number of cation exchange equivalents and express it in meq/100 g of soil
Calculated solely at 25 Celsius of PbCrO4 in pure water and in a .0130M. Na2CrO4 solution. Ksp of PbCrO4 is 2.8x10^-13
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?
For a 0.1 M aqueous solution of sodium acetate, NaCH3CO2, one mass balance is simply [Na] 0.1 M. Write a mass balance involving acetate.
The distribution coefficient (K) of formic acid (HCO2H) in 1-octanol versus water is 0.39. If a solution of 4.00 grams of formic acid in 100.00 mL of 1-octanol is extracted with one 10.00 mL portion of water, how many grams (to the hundredths place) will remain in the organic layer?