Test3

11. Refer to the attached photo. Thank you!

2. Consider the reaction of cyanide ion (CN) with water, where cyanide ion is either a weak acid or a weak base. a) Select the correct chemical equation for the acid/base dissociation reaction of cyanide ion in water: OCN- (aq) + H₂O (/) HCN (aq) + H3O+ (aq) OCN- (aq) + H₂O (/) = H₂CN+ (aq) + OH¯ (aq) OCN- (aq) + H₂O (/) = H₂CN+ (aq) + H3O+ (aq) OCN- (aq) + H₂O (/) HCN (aq) + OH- (aq) Incorrect. Tries 3/3 Previous Tries b) The equilibrium expression for this reaction corresponds to: Incorrect Ka Correct: Kb You are correct. Previous Tries Your receipt no. is 152-2641 c) The numerator of the equilibrium expression (from part b) for this reaction is: [HCN ] O[ H₂CN+ ][ OH-] O[OH ][ HCN ] [H₂CN+ ] O[ HCN ][ H3O+] O[H3O+] O[H₂CN+ ][ H3O+] O[OH ][ CN¯ ]

Calculate the pH of the resulting solution if 22.0 mL of 0.220 M HCI(aq) is added to 32.0 mL of 0.220 M NaOH(aq). pH = Calculate the pH of the resulting solution if 22.0 mL of 0.220 M HCI(aq) is added to 12.0 mL of 0.320 M NaOH(aq). pH = Connect CAPS Charg #3 $ % & 4. 5 6 7 W Y J K X N M Alt Command Command Option Home * CO

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.735, the hydrogen ion concentration is mol/L.

ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?

In the following acid-base equilibria of weak acids in water, label the acid (A), the base (B), the conjugate acid (CA), and the conjugate base (CB). HCIO, (aq) + H,O(1) = H,O*(aq) + CI0, (aq) H,CO, (aq) + H,O1) – H;O*(aq) + HCO; (aq) Answer Bank H,O(1) + CH;NH†(aq) = CH,NH,(aq) + H;O*(aq) СА А B СВ CH, COOH(aq) + H,O(1) - CH;COO (aq) + H;O*(aq)

Complete the balanced molecular reaction for the following weak acid with a strong base: HF(aq) + LIOH(aq) – 4+ 1 8 O2 03 04 O5 口 口 6. (s) (1) (g) (aq) Li H2O OH H3O* H. Reset • x H2O Delete 3.

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.

1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.

3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.

The pH of an aqueous solution of acetic acid (CH,COOH) is 2.5229. What is the initial molar concentration of HCOOH, if its acid ionization constant is K, = 1.8x10°? Enter a your answer in the box provided with correct units and sig. figs.: The initial molar [CH,COOH], = Answer: concentration of : %3D acetic acid is

Choose the right variant of reaction when the following strong acid and strong base react with each other: a. HCl(aq) + RbOH(aq) → Mastered OHCl(aq) + RbOH(aq) → H₂O(1) + RbCl(s) O 2HCl(aq) + RbOH(aq) → H₂O(1) + RbCl₂ (aq) O HCl(aq) + 2RbOH(aq) → H₂O(1) + Rb₂ Cl(aq) O HCl(aq) + RbOH(aq) → H₂O(1) + RbCl(aq) b. HC1O4 (aq) + NaOH(aq) → [Review Topics] OHCIO4 (aq) + NaOH(aq) → H₂O(l) + NaClO4 (aq) OHC1O4 (aq) + 2NaOH(aq) → H₂O(1) + Na₂C1O4 (aq) HC1O4 (aq) + 3NaOH(aq) → H₂O(l) + Na3 C1O4 (aq) OHCIO4 (aq) + NaOH(aq) → H₂O(l) + NaClO4 (8) c. H₂SO4 (aq) + NaOH(aq) → H₂SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + 2H₂O(1) O H₂SO4 (aq) + NaOH(aq) → Na2SO4 (aq) + H₂O(l) O H₂SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + H₂O(l) H₂SO4 (aq) + 2NaOH(aq) → Na2SO4 (8) + 2H₂O(1) Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous S

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. H₂S (aq) + KOH(aq) → 2- 3C₂² 1 2 + (s) S 3 K Reset 4 (1) 5 6 LO O 7 (g) ㅈ H 8 9 11 (aq) Submit X 0 • x H₂O

Calculate the pH of the resulting solution if 34.0 mL of 0.340 M HCl(aq) is added to 44.0 mL of 0.340 M NaOH(aq). pH = Calculate the pH of the resulting solution if 34.0 mL of 0.340 M HCl(aq) is added to 24.0 mL of 0.440 M NaOH(aq). pH = OCT MacBook Pro & Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Scien

The value of crotonic acid is 2.04 x 10^-5

Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid:   HClaq        à               H+aq     +          Cl-aq   and convert the following expression to deduce the hydrogen ion concentration:   pH = -log10 [H+]     (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3