The following reaction (Keq = 1.8 × 10−5) starts with 0.100 M HC2H3O2, with all other aqueous species zero molar. What is the final concentration of H3O+? HC2H3O2(aq) + H2O(l) — H30+(aq) + C2H3O2(aq) H¸O±(aq)
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- What is the net ionic reaction of HNO3 (a strong acid) with KOH (a strong base)? H2O (0)→ H+ (aq) + OH (aq) H+ (aq) + OH- (aq) → H₂O (1) HNO3(aq) + KOH (aq) → KNO3 (aq) + H₂O (1) K+ (aq) NO3(aq) →>> KNO3(aq)The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)Phosphoric acid, H3PO4, is a polyprotic acid. What is the THIRD ionization reaction for phosphoric acid in water? HPO (aq) → H+ (aq) + PO³ (aq) ○ H3PO4 (aq) → 3 H+ (aq) + PO¾- (aq) 4 H₂PO (aq) → HPO²¼¯ (aq) + H+ (aq) H3PO4 (aq) → H₂PO (aq) + H+ (aq)
- More H3O+ ions are added to an HCN and CN- buffer solution. Which reaction will occur to neutralize the additional H+ ions? H3O+ (aq) = HCN (aq) + H2O (1) HCN (aq) + H2O (l) = CN¯ (aq) + H3O+ (aq) H3O+ (aq) = CN¯ (aq) + H3O+ (aq) CN¯ (aq) + H3O+ (aq) = HCN (aq) + H₂O (1)Adding acid to the buffer, NH3-NH4*, will produce this (net ionic) reaction: H*(aq) +OH(aq)=H₂O(1) H*(aq)+NH4*(aq) NH3(aq)+H₂(g) O H*(aq) + NH4+ (aq)=NH5²+ (aq) O H*(aq)+NH3(aq)=NH4+ (aq)The following reaction (Keq = 1.8 × 10−5) starts with 0.100 M HC2H3O2, with all other aqueous species zero molar. What is the final concentration of H3O+? HC2H3O2(aq) + H2O(l) — H30+(aq) + C2H3O2(aq) H¸O±(aq)
- The following reaction (Keq = 1.8 × 10−5) starts with 0.100 M HC2H3O2, with all other aqueous species zero molar. What is the final concentration of H3O+? HC2H3O2(aq) + H2O(1) H3O+ (aq) + C2H3O2(aq)Information given= Reaction #2: (K+(aq) + OH-(aq) + (H+)+(aq) + Cl-(aq) → K+(aq) + Cl-(aq) +H2O(l) Mass of empty cup in grams (tare mass) 1.764g Mass of cup+solution (g) 30.128g Temp of HCI solution in (c) 21 degree celsius Temp of KOH solution (c) 22 degree celsius Time (seconds) Temp ( in degrees celsius 30 24 60 24 90 24 120 24 150 24.5 180 24.5 Question 1: From the 6 or 7 initial temperatures collected, calculate the average ΔTi.A weak acid has a Ka of 7.6 x 106. What is the value of pk for the acid? a pKa =
- H2SO4 (aq) + 2 NaOH (aq) Na2SO4 (aq) + 2 H2O (l) calculate the molarity of the H2SO4 solution if 14.92 mL of NaOH was necessary to reach the endpoint of a titration. The molarity of the NaOH solution was 0.63 M and 25.18 mL of H2SO4 was added to the Erlenmeyer flask.Open bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water. The dissolution of carbon dioxide produces carbonic acid (H2CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO2 (g) + H2O (l) H2CO3 (aq) H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq) The equilibrium between carbonic acid (H2CO3) and bicarbonate (HCO3-) is influenced by the presence of dissolved metals from the bedrock underlying a body of water. Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal. The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure). Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic acid/bicarbonate equilibrium?A buffer solution made from nitrous acid and sodium nitrite was titrated with sodium hydroxide. What is the net ionic equation for the reaction?