6. Classify the following salts as acidic/basic/pH neutral and write a hydrolysis equation for them where appropriate. salt Acidic/basic/neutral Hydrolysis equation if applicable CsF NHẠCI 7. Write the conjugate acid (if any) of each of the following: a. H2PO4 b. ОН 8. The Ksp for CaF2 is 2.00 x 10-10. a. Calculate the molar solubility in pure water. b. Calculate the solubility of CaF2 in 0.080 M KF.

6. Classify the following salts as acidic/basic/pH neutral and write a hydrolysis equation for them where appropriate. salt Acidic/basic/neutral Hydrolysis equation if applicable CsF NHẠCI 7. Write the conjugate acid (if any) of each of the following: a. H2PO4 b. ОН 8. The Ksp for CaF2 is 2.00 x 10-10. a. Calculate the molar solubility in pure water. b. Calculate the solubility of CaF2 in 0.080 M KF.

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

Calculate the percent lonization. of acetic acid in a solution that is 0.2014 in acid (HC₂H30₂) and 0.20m z Oz in potassium actate (KC z H z O ₂ ) z The acid dissociation constant of acetic acid is 1.8x10-5. 0 5.6% 0.000912 0 0.38% O 12% 0.0 27%
Pls help ASAP
+ Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+]. PK₂ is the negative logarithm of Ka. PK₂ -log Ka The Henderson-Hasselbalch equation is used buffer solutions: calculate the pH of base DAGSK pH =pK₂ +log acid] Notice that the pH of a buffer has a value close to the PK₂ of the acid. differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and PKb is similar. acid [base pOH = pkt + log- Part A Acetic acid has a K₁ of 1.8 x 105. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate]. B. [acetate] ten times greater than [acetic acid], and c. [acetate] [acetic acid]. Match each buffer to the expected pH Drag the appropriate items to their respective bins. ▸ View Available Hint(s) [acetic acid] ten times greater than [acetate] pH = 3.74 [acetate] ten times greater than [acetic acid] pH = 4.74 Reset Help…
26 162 1. pH Buffers are solutions that contain mixtures at similar concentrations of a weak acid and its conjugate base. Below are conjugate acid-base pairs that can be used to make pH buffers in this lab. For each pair, label the weak acid and the conjugate base. buffer 1: buffer 2: buffer 3: NH3 CH3COOH Name: HPO4²- NH4* CH3COO H₂PO4
Clear my choice A student dissolve 1.0 g of a mixture containing benzoic acid, p-methylaniline and cholobenzene in 20.0 mL of 10% HCL solution. After separating two layers, he added 10% NaOH to the aqueos layer until basic to litmus paper. The Precipitate formed is : O a. chlorobenzene O b. p-methylaniline and benzoic acid Oc. p-methylaniline O d. benzoic acid NEXT PAGE Jump to... Announcements TOSHIBA IN & 6 7 7 V 8 A FIGY Hi
Help! Please solve Q5 all parts
0.10 HC2H3O2 2.910.010 HC2H3O2 3.350.0010 M HC2H3O2 3.73 1. Write the net ionic equation describing the dissociation ofacetic acid in aqueous solution.2. Calculate [H+] and[ C2H3O2-] for each concentration above, showing a sample calculation here.3. Write the equilibrium constant expression for acetic acid, andcalculate a K value and an apparent percent dissociation for eachconcentration showing sample calculations.
If a 0.10 M aqueous solution of a weak monoprotic acid (HA) is 5.0% dissociated (i.e. aA. = 0.05), what is the %3D acid equilibrium constant, Ka, for this acid? The reaction involved is: HA + H20 H30+ + A a. 2.5 x 10-4 b. 5.0 x 10-2 c. 5.0 x 10-3 d. 2.5 x 10-5
1. Adding NaCl to: HC₂H₃O₂ + H₂O ↔ C₂H₃O₂⁻ + H₃O⁺ a. reaction shift backward b.reaction shift forward c.no effect d.none of the above 2.A stock solution has a concentration of 0.05 M. Which of the following concentrations might be the concentration of the final solution when diluted? 3.A buffer system with pKa of 6.4. Which of the following pH is reasonable when a base is added to the buffer solution?
Pls help ASAP
Acetic acid has a Ka of 1.8 x 10-5. Three acetifc acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate] B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid]. Match each buffer solution to the expected pH: a) pH = 3.74 b) pH = 4.74 c) pH = 5.74
Write out the dominant chemical reaction/equilibrium that wil determine solution pH when 0.1 mole of each of the following compounds is dissolved in 1 L water. DO NOT CALCULATE pH. a. Na[CH3CH2CO2] b. HC104 c. (CH3)3N d. HS CH2OH