X02-After-Lab

Suppose sodium hydroxide is added to a 0.0120 M solution of zinc nitrate such that the pH of the solution is 13.1. What is the equilibrium concentration of Zn2+? Zn2+(aq) + 40H (aq) Zn(OH)42-(aq); Kf = 2.8 x 1015 1.70 x 10-14 M 00 × 10¬14 M 9.06 x 10-15 M O 1.22 x 10-14 M 8.40 x 10-15 M

What is the correct equilibrium constant expression for the following reaction? NH3(aq) + H₂O(NH4+ (aq) + OH(aq) [NH3] [H₂O] [NH4]+[OH]- (A) Kc = (B) K (C) Kc (D) Kc (E) Kc = = = = - [NH₂+] [OH-] [NH3] [NH4+] [OH [NH3] [H₂O] [NH3] [NH4+] [OH [NH₁+]+[OH-] [NH3]

Write the chemical equation

1) Gallium hydroxide, Ga(OH)3, has a KSP of 7.28x10-36. Ga(OH)3(s) ⇌ Ga3+(aq) + 3OH-(aq)Under which circumstance will the [Ga3+] be the highest? Justify your answer.A) Dissolved into 1.00 L distilled waterB) Dissolved into 1.00 L of 1.00 M HClC) Dissolved into 1.00 L of 1.00 M NaOH

A(NH3)3+ is a complex ion. A+(aq) + NH3(aq) ⇌ ANH3+(aq).                 K 1 = 3.3 x 10^3 ANH3+(aq) + NH3(aq) ⇌ A(NH3)2+(aq)      K2 = 6.4 x 10^3 A(NH3)2+(aq) + NH3(aq) ⇌ A(NH3)3+(aq) K3 = 1.2 x 10^3 Calculate the equilibrium concentrations of all species in solution, including the spectator ions, NH4+, OH−, and H+, if 100.0 mL of 0.100 M ANO3 is added to 300.0 mL of 2.0 M NH3.

Carbonate (H2CO3/HCO3-) buffers are important in regulating the pH of blood at 7.40.  Note that the Ka for H2CO3 is 4.3 x 10-7. When a person exercises, muscle contractions produce lactic acid.  Moderate increases in lactic acid can be handled by the blood buffers without decreasing the pH of blood.  However, excessive amounts of lactic acid can overload the blood buffer system, resulting in a condition called acidosis if the blood pH falls to 7.35 or lower. Suppose a patient’s normal blood sample contains [H2CO3] = 0.0015 M and [HCO3-] = 0.0129 M.  If this patient exercises enough to produce 0.0010 mole of H3O+ per 1 L of blood due to production of lactic acid, would they be diagnosed with acidosis?

Given the two reactions 1. H2 S(aq) = HS-(aq)+ H+(aq), K1 = 9.38×10-8, and 2. HS (aq) = S²- (aq) +H†(aq), K2 = 1.16x10-19, what is the equilibrium constant Kfinal for the following reaction? S²-(aq) + 2H†(aq) = H2S(aq)

Predict the products of each reaction, and whether the solution at equilibrium will be acidic, basic, or neutral. At equilibrium the solution is...? reaction acidic N,0,(s) + 3H,0(1) → 0 basic neutral O acidic co, (g) + H,0(1) basic neutral acidic Na, 0 (s) + H,0(1) - 0 basic neutral

ys 111111

Give good solution

2 Ht +H2O2 + 2 Fe2+ 2 Fe3+ + 2 H2O in acidic solution

2+ Given Ca²+ (aq) + CO3²−(aq) ⇒ CaCO3( s), Kc =2.2 × 10⁹. What is the value of the equilibrium constant for CaCO3(s) ≤ Ca²+ (aq) + 2- CO3²- (aq)? 2.2 × 108 4.5 × 10-⁹ -2.2 × 108 4.5 × 10⁹ 2.2 x 107 -8

Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. HCIO,(aq) – 4- 2- n2+ 3+ D 4+ + 1 3 4 6. 7 8 Os O8 (s) (1) (g) (aq) NR CI Reset • x H,O Delete x H̟O 2 11 3. 2. +

COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…

Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]

Supply the missing data in the tables below. Acid Molar Analytical Concentration, CT (CT = = CHA + CA-) pH [HA] [A¯] αo αι Lactic Ka = 1.38 × 10-4 0.118 0.622 3 10-4) M (Ka = 1.7 x Iodic Ka 0.290 < 10-¹) CULO 3 0.750 M

Write the chemical formula for diphosphorus pentabromide 3- |2+ 3+ 4+ 1 2. 3. 4 9. 7 8. 9. O2 3 Os 1 6. lo (s) (1) (g) (aq) В Ph Br Po Pm Reset • x H2O Delete P.

55. Human blood is buffered by carbonic acid and bicarbonate ions. Alkalosis is a condition caused by excess production of bicar- bonate in the blood. A patient's blood plasma has a pH = 7.6 (pKa for H2CO3 at body temperature is 6.1). MISSED THIS? Read Section 18.2; Watch KCV 18.2B, IWE 18.2, 18.3 [HCO3] [H2CO3] a. What is the ratio of in the patient's blood? b. The doctor gives the patient 0.45 g of HCl intravenously to neutralize alkalosis. After treatment, the patient's blood is 0.0156 M in HCO3¯ and 0.0012 M in H2CO3. If the volume of blood in the patient's body is 5.3 L, what is its new pH?

(CH3)2O →BF3(g)⇋BF3(g)+(CH3)2O(g) If you place 1.2 g of the complex in a 61.5 mL flask at 125 ℃, what is the total pressure in the flask at equilibrium? What are the partial pressures of the Lewis Acid, Lewis Base, and the complex? (Given: The value of K (here Kp) for the reaction is 0.17 at 125 ℃.) P(BF3)= P((CH3)2O)= P((CH3)2O→BF3)=

Write the basic equilibrium equation for PO43 04- 2. | 2+ 3+ O 4+ 2 3 4 7 8 9. O2 O5 (s) (1) (g) | (aq) + + H3O* H. H2O OH Reset • x H2O Delete + 3.