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Consider the buffer solution: HNO3(aq) + H20(1) -- NO2 (aq) + H30*(aq) What happens to the...
Consider the buffer solution: HNO3(aq) + H2O(1) - NO2 (aq) +H30*(aq) What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
Consider the buffer solution: HNO2(aq) + H2O(l) + NO2 (aq) + H30+(aq) • What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
Consider the buffer solution: HNO2(aq) + H2O(l) + NO2 (aq) +H30+(aq) What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
explain why please 3. Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO3(aq) +H2O(l) — H30*(aq) + NO2 (aq) In which direction will the equilibrium shift if -a. NaOH is added? right diplllspintado 2102 b. NaNO, is added? Shift to Wt to cleanace NO2 - C. HCI is added? Just d. The acid solution is made more dilute? OM assumen d ie da .
OD.HNO3 O E. H20 QUESTION 11 Consider the reaction HNO2(aq) + H2O(0-14.10-H30+(aq) + NO2-(aq). Which species is a conjugate base? O A HNO2(aq) O B. H200) O C H30 (oa) No2 (aq) two of these QUESTION 12 tion contains 0.25 M HF and 0.79 M NaF A 1.0-liten ng system:
Consider a buffer solution whose acid component is nitrous acid, HNO2 a) what is a conjugate base component of this buffer? b) write a reaction that takes place when a small amount of H3O+ is introduced to this buffer solution. c) write a reaction that takes place when a small amount of OH- is introduced to this buffer solution
23) Consider the following generalized buffer solution equilibrium: BH+(aq) + H2O(1) H3O+(aq) + B(aq) 24) Select the ionic compound that is insoluble in water. A) Fe(NO3)3 B) MgS C) KBr D) NaCO3 E) NH_Br Consider the following generalized buffer solution equilibrium: BH+(aq) + H2O(1) H3O+(aq) + B(aq) When a small amount of a strong base such as sodium hydroxide is added to ti solution, which of the four species shown would experience an increase in concentration? (Hint: Use LeChatelier's principle.)...
help with these chemistry questions 1. Explain what happens to the concentration of H,O' ions in an acetic acid solution when solid sodium acetate is added. 2. Determine the pH and pH of a solution that is 0.5 M NaHSO4 and 0.25 M Na2SO4 3. When sodium nitrite is added to HNO2(aq) a) the equilibrium concentration of HCOOH(aq) decreases. b) the pH of the solution increases. c) the K increases. d) the pH of the solution does not change. e)...
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq) + C3H502 (aq) The value for the acid-dissociation constant for propionic acid (HC3H502) is 1.3x10-5 at 25°C. Calculate the hydronium ion concentration present in a propionic acid solution that has the following equilibrium concentrations. 3.24x10-2 mol/L HC3H502 3.06x10-4 mol/L for propionic acid's conjugate base, C3H5027 The general form of the acid-dissociation constant is Ka = [H30'A ], where Ka is the acid-dissociation constant, [HA]...
Question 3 1 pts Which statement accurately describes what happens in a buffer solution when you add strong acid or strong base? The strong species is converted to weak species by reaction The pH change is smaller than you expect based on the amount of acid or base added Two reactions occurs-first a completion reaction, then an equilibrium reaction All three statements above accurately describe this situation Question 4 Can you create a buffer by mixing HNO3 with KOH? Yes-...