Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. HONH,NO, 04- O4+ 3. 4 6. 8. 1 2 04 9. (s) (1) (g) (aq) H. NR H,O OH C N Reset • æ HO Delete 9,

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. HONH,NO, 04- O4+ 3. 4 6. 8. 1 2 04 9. (s) (1) (g) (aq) H. NR H,O OH C N Reset • æ HO Delete 9,

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 3RQ

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For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. (CH:):NH2CIO4 2+ 13+ 14+ 1 2 3 4 5 7 8 9 Do (1) (g) (aq) H NR C OH- H2O CI N CO LO 3. 4.
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. NH&Br 14- |3- O2+ 3+ 4+ 1 2 4 6. 7 8 9. Os 18 Do ) (s) (1) (g) (aq) Br OH- H3O- H2O NR Reset • x H2O Delete 1L +
Q1 A mixture of acetic acid and sodium acetate makes an effective buffer. Here is the equilibrium equation for these two species: HC,H3O2 (aq) + H2O (I) = C,H3O2¯ (aq) + H3O† (aq) (a) What reaction would take place if acid were added to this buffer? (b) What reaction would take place if base were added to this buffer?
Question 4 of 11 Submit Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. CsC,H,O6 3c,2- Reset > 1 2 3 4 5 7 8 + (s) (1) (g) (aq) H2O NR C Cs H3O* OH- • x H20 LO
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. C5H;NHI 2- + 2+ 3+ 4+ 1 2 3 4 6. 7 8 9 1 3 04 O6 O7 + (s) (1) (g) (aq) C OH H. NR H2O H30* N Reset • x H2O Delete LO 3.
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. CSHSNHI 04- D2+ 3+ 4+ 1 2 4 5 7 9 3 Os (s) (1) (g) (aq) + OH- NR H H3O+ C H2O Reset • x H2O Delete CO LO
Kc for formic acid dissociation in water is 1.8x10-4. What are the equilibrium concentrations of H30+ HCOO- and HCOOH if the initial concentration of HCOOH is .15 mol? HCOOH (aq) +H20 (L) >< H30 (aq) + HCOO (aq)
Write the balanced NET IONIC equation for the reaction that occurs when hydrobromic acid and sodium hydroxide are combined. Use H3O+ instead of H+. (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g) This reaction is classified as.A. Strong Acid + Strong BaseB. Weak Acid + Strong BaseC. Strong Acid + Weak BaseD. Weak Acid + Weak BaseThe extent of this reaction is:.A. ... Below 50%B. ... 50%C. ... Above 50%D. ... 100%
Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENT

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