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

Mass balance equation based on the law of conservation of mass.According to this all the species…

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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Solution 1) 50.00mL of a solution containing 0.15M malonic acid, CH2(CO2H)2, and 0.020M manganese (II) sulfate, MnSO4. Calculate the mass (in grams) of manganese(II) sulfate monohydrate required to prepare solution 1. Your answer should have 2 sig figs.
Calculate the number of moles of K+ and CO3 2- ions in 25 cm3 of 0.20 M K2CO3 solution.
What is the molar concentration of silver ion, Ag*(aq), in a 1.00 M solution of Ag(NH3)2 with no excess ammonia? (K= 1.70 x 107 for Ag(NH3)2*)(round to one decimals, after writing the number, leave a space and write the units)
What is the pH of a solution that is a prepared by dissolving 4.90 g of (NH4)2SO4 ( K₁ (NH4+) = 5.70 × 10-¹0) in water, adding 150.0 mL of 0.1263 M NaOH, and diluting to 900.0 mL? pH = b0.124 M in piperidine and 0.054 M in its chloride salt ( Ka (C5H₁1NH+) = 7.50 × 10−¹² )? -12 pH = C prepared by dissolving 2.12 g of aniline (93.13 g/mol, Ką (anilinium ion) = 2.51 × 10−5) in 100. mL of 0.0330 M HCl and diluting to 500.0 mL? pH =
Calculate the equilibrium molarity of aqueous Hg^2+ ion. Round to Two sig figs.
You may want to reference (Page 834) Section 18.3 while completing this problem. Part A If 130.0 mL of 0.0020 M Na2SO4 (aq) is saturated with CaSO4, how many grams of CaSO4 would be present in the solution? [Hint. Does the usual simplifying assumption hold?] Express your answer using two significant figures. VE ΑΣΦ ? m = 0.43 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining g
What is the equilibrium constant value for NaC2H3O2 and how do you find its Kb?
3.A sample is known to contain NaOH, NA2CO3 NaHCO3 or compatible mixture of these together with inert matter. With methyl orange, a 1.100 g sample requires 31.40 mL of HCI ( 1.00 mL is equivalent to 0.0140g CaO). With phenolphthalein indicator, the same weight of sample requires 13.30mL of the acid. What is the percent composition of the sample?
Ascorbic acid (H₂C,H,O) is a diprotic acid. The acid dissocation constants for H₂C,H,O, are Kal = 8.00 x 10-5 and K₁2 = 1.60 x 10-12 Determine the pH of a 0.117 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H₂C,H,O,] = [HC,H,O,]= [C,H,O2] = M M M
Which salt would you expect to dissolve readily in acidic solution, calcium phosphate, Ca3(PO4)2, or calcium sulfate, CaSO4? Give a full and clear explanation.
Calculate the concentration, in mol/L, of a saturated aqueous solution of Ag3P04 (Ksp = 1.80×10¯18). 1.61×10 mol/L You are correct. Calculate the solubility, in g/100mL, of A93PO4. 6.73x104 g/100mL You are correct. Calculate the mass of Pb3(PO4)2 (Ksp = 1.00x10-54) which will dissolve in 100 ml of water. Submit Answer Tries 0/5 Rank the following five salts in order of decreasing solubility, in terms of mass per unit volume. (The most soluble gets rank 1, the least soluble gets rank 5.) v Cas(PO4)3F (Ksp = 1.00x10-60) (Ksp = 1.50x10-9) (Ksp = 1.20x10-5) (Ksp = 1.00x10-54) (Ksp = 1.80x10-18) v BaSO4 Ag2SO4 Pb3(PO4)2 v A93PO4
From the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)