None 18. If ionic species in a neutral solution (pH=7) ofCaCl2 are Ca2+, Cl, CaCl, and CaOH+, the massbalance equation is:a. [CI] + [CaC1] = 2x {[Ca2+] + [CaC1*] +[CaOH+]}b. [CI] = 2 × [Ca2+] + [CaC1] + [CaOH+][CI] + [CaC1] + [Ca(OH)2] = 2 × {[Ca2+] +[CaC1]+[CaOH+]}C.d.[Cl] + [CaC1] = 2 × {[Ca2+] + [CaCl*] +[CaOH+]+[Ca(OH)2}Show work. don't giveHandwritten answer

[Cl]: This represents the concentration of chloride ions in the solution.[CaCl+]: This represents…

Answered: 18. If ionic species in a neutral…

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...

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Buffers are solutions that buffer against large changes in pH when an acid or base is added. Buffers contain a weak acid to neutralize added base, and a weak base to neutralize added acid. Most buffer problems want you to calculate the pH. For example, Calculate the pH of a buffer made from dihydrogen phosphate and hydrogen phosphate when the [H2PO4-1] = 4.44 x 10-5 M, the [HPO4-2] = 5.55 x 10-5 M, and the Ka = 6.20 x 10-8.
The titration of 25.0 mL of a mixture of hydrochloric acid and formic acid (HCO,H) with 0.78 M NAOH gave the titration curve below. Like HCI, formic acid is also monoprotic. What are the molarities of HCl and HCO2H in the solution? 12.0 11.0 10.0 9.0 8.0 7.0 PH 6.0 5.0 4.0 3.0 2.0 1.0 5.0 10.0 15.0 20.0 25.0 30.0 Volume (mL)
Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = Units
A solution is made by mixing exactly 500 mL of 0.156 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8×10−5 [H+] M Enter your answer in scientific notation. [OH−] M [CH3COOH] M Enter your answer in scientific notation. [Na+] M [CH3COO−] M
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC,H,O2 is 1.5 x 10-5. 3 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base You can ignore the amount of liquid water in the reaction. HC4H,O2(aq) OH (aq) H2O(1) C4H,O2 (aq) + Before (mol) 1.00 x 103 8.00 x 103 8.00 x 103 Change (mol) -2.00 x 103 -8.00 x 103 After (mol) 8.00 x 103 6.00 x 103 2.00 x 103 RESET 0.100 0.200 1.00 x 103 -1.00 x 103 2.00 x 103 -2.00 x 103 6.00 x 103 -6.00 x 103 7.00 x 103 -7.00 x 10"3 8.00 x 103 -8.00 x 10"3
1) A buffer solution is 0.337 M in H2CO3 and 0.239 M in KHCO3 . If Ka1 for H2CO3 is 4.2x10^-7 , what is the pH of this buffer solution? pH = 2) An aqueous solution contains 0.302 M hypochlorous acid. How many mL of 0.231 M potassium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 7.540? 3) 36.5 mL sample of a 0.310 M aqueous hypochlorous acid solution is titrated with a 0.441 M aqueous barium hydroxide solution. What is the pH after 8.80 mL of base have been added? Ka for HClO is 3.5x10^-8 . pH =
A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C₆H₅NH₃⁺ in the solution. The value of Kb for C₆H₅NH₂ is 3.8 × 10⁻¹⁰. Let x equal the original concentration of C₆H₅NH₃⁺ in the water. Based on the values given, set up an ice table to determine the unknown. Based on the ice table, set up the expression of Kb in order to determine the unknown. Do not simplify or combine terms. Based on the ice table and kb expression, determine the original concentration of C₆H₅NH₃⁺.
Calculate the pH of a solution in which 15 mL of 0.10 M NaOH is added to 25 mL of 0.10M HCI. A 1.24 g sample of benzoic acid, C6HSCOOH was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.180M NAOH. What was the pH of solution when the equivalence point was reached? Ka CeHsCOOH = 6.3 x 10-5 Draw the pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition of 0.10 M HCI from the burrete. Label the axes and put a scale on each axes. Show the equivalence point and buffer region. K, NH3 = 5.6 x 10-10
Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka = 2.8 x 109) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 82.86 g KOBr and 250 mL of 1.50 M HOBr, and adds enough distilled water to make 925 mL of solution. What is the pH of this solution? pH solution = Part 2 Next, Lareina adds 16.0 mL of 2.20 M HNO₂ to 350 mL of the solution made in Part 1. What is the pH of the solution after the HNO, is added? pH after HNO, added = Part 3 Finally, Lareina 16.0 mL of 2.00 M NaOH ito 395 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added= =
pH Titration A student is titrating 150.0 mL of a 0.300 M solution of lactic acid (pKa of lactic acid is 3.85) with a 0.250 M solution of NaOH. Calculate the initial pH of the lactic acid solution, before any NaOH has been added. Round your answer to 2 decimal places. pH = Calculate the pH of the acid solution after the chemist has added 100.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH = Calculate the pH of the acid solution after the chemist has added 200.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH =
- Calculate the pH of a 1.00 L buffer solution containing 0.143 mol of acetic acid (HC₂H30₂) and 0.180 mol of sodium acetate (NaC₂H₂O₂). The Ka of acetic acid is 1.8 × 10-5. pH = Calculate the pH of the buffer solution after 0.0315 mol of HCl is added to the buffer. Assume the volume of the solution does not change. pH = Calculate the pH after 0.0315 mol of HCl is added to 1.00 L of pure water. pH =
A buffer is created by mixing equal concentrations of NH4+ and NH3. Calculate the volume of the NH4+ solution (in mL) needed to create a buffer of pH = 8.89 with a total volume of 126 mL. Kb (NH3) = 1.80 x 10-5 Answer to 1 decimal place.

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