Can you include the species please 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 existswhen the salt is dissolved in aqueous solution. If neutral, simply write onlyNR. Be sure to include the proper phases for all species within the reaction.KC3H5O34-2-2+3+☐ -ப☐4+12 34567890☐☐ 2☐ 345☐ 6☐7☐8☐ 9口。+)14(s)(aq)tvADII40F8F780F6F5FA44F9'CF10

Step 1:KC3H5O3 is potassium lactate. It will dissociate to potassium ions (K+ ) and lactate ions (…

Answered: Determine if the following salt is…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.DCP

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The reaction just described is reversible. Deprotonation of the conjugate acid of an organic base by water provides another example of simultaneous making and breaking of sigma bonds. Thus, in the deprotonation of anilinium ion by water, the base is water, which has unshared electrons on the ________ atom. The acid is ________ ion. A pair of ________ electrons on the oxygen atom of water is pushed toward the ________ atom. Simultaneously, the pair of ________ electrons between the hydrogen and ________ atom of the anilinium ion is pushed toward the ________ atom. Thus, the oxygen- ________ sigma bond is made and a hydrogen- ________ sigma bond is broken. The nitrogen atom, which possessed a positive charge, is now ________, and the oxygen atom, which was neutral, now possesses a formal ________ charge.
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
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
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
When the reversible reaction HC2H;O2 (aq) E> H(aq) + C2H3O2 (aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of NaOH (aq) to the reaction mixture? a) pH will not change because NaOH is not a part of the reaction equation. b) pH will not change because acetic acid and NaOH form a buffer. c) pH will increase because NaOH will completely neutralize acetic acid. d) pH will decrease because NaOH will completely neutralize acetic acid. In the reversible reaction A (aq) + B(aq) E > C(aq), reactant A is very expensive. What are two ways to get it to react as fully as possible to form as much C as possible? a) remove C as it forms, and use an excess of A b) add another reactant that will form a precipitate with B c) remove C as it forms, and use an excess of B d) add another reactant that will form a precipitate with A
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. Be sure to include the proper phases for all species within the reaction. Lil k + 4- Π 2+ 3+ 4+ 2 3 4 5 6 7 8 9 0 ப 2 ☐ 3 4 Π 6 07 8 9 0 ) = (s) (1) (g) (aq) APR Science Chemistry C tv AQ
13. Consider the following acids and their dissociation constants: HPO,2- (aq) + H2O(1) → H3O* (aq) + PO2* (aq) K= 2.2 x 10-13 HCHO2(aq) + H2O(1) H3O*(aq) + CHO2'(aq) K= 1.8 x 104 (a) Which is the weaker acid, HPO,²- or HCHO2? (b) What is the conjugate base of HPO42-? (c) Which acid has the weaker conjugate base? (d) Which acid has the stronger conjugate base? (e) Which acid produces more ions? solutien 0.02 arco
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. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.
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. Be sure to include the proper phases for all species within the reaction. Ba(CHO) Ba(CHOz)z(aq) + 2 H2O(I)= Baz+(aq) + 2 CHO, (aq) + 2 OH-(aq)
6. Determine the Gibb's free energy of a reaction system which consists of 0.6M monoprotic acid, 0.6M conjugate base, and has a pH = 3.5. 7. Determine the Gibb's free energy of a reaction system which consists of 2 mol NOBI, 1 mol NO and 1 mol Br2 in a 2 L vessel at 30°C. The equilibrium constant (KC) at this temperature is 15. 2NOBr(g) 2NO(g) + Br2(g)
Use systematic treatment of equilibrium to solve this problem and determine the pH. STEP by STEP f. A 100 mM solution of ammonium acetate (CH3COO NH4). Use activity coefficients. NH4+ (aq) NH3(aq) + H+ (aq) 1 Ka= 5.69 x 10-10 CH₂COOH(aq) → CH3COO- (aq) + H+ (aq) Ka = 1.75 x 10-5
1) Write the equilibrium constant expression for the following reaction. CaO(S) + 2HCl (aq) <=>CaCl2 (aq) + H2O(l) 2) At 90 C , Kw is about 10-13, what is the pH under these conditions? 3. Will an aqueous solution of NaCl be acidic, neutral or basic?

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