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)
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A: Step 1: GivenHC2H3O2 (aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Keq = 1 .8 * 10−5 [HC2H3O2] = 0.100…
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- 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)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)
- NaCLO(s) dissociates when it dissolves in water: NaClO(s) + H2O(l) →Na+(aq) + ClO−(aq) and in water ClO− acts as a base with a conjugate acid of HClO(aq) ClO- (aq) + H2O(l) = HClO(aq) + OH- How much NaClO must be added to 2.00L of water to make make a solution with a pH=11.0? Kb=[HClO][OH−]/[ClO−] =3.3x 10−7More 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)
- A weak acid has a Ka of 7.6 x 106. What is the value of pk for the acid? a pKa =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)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?
- Write and balance the following acid-base neutralization reaction:HBr(aq) + Li2CO3(aq) →→ Write and balance the following acid-base neutralization reaction:HBr(aq) + Li2CO3(aq) HBr(aq) + Li2CO3(aq) →→ LiBr(aq) + H2O(l) + CO2(g) 2 HBr(aq) + Li2CO3(aq) →→ 2 LiBr(aq) + H2O(l) + CO2(g) HBr(aq) + Li2CO3(aq) →→ 2 LiBr(aq) + H2CO3(l) 4 HBr(aq) + Li2CO3(aq) →→ 2 LiBr2(aq) + 2 H2O(l) + CO2(g)HelpWhich of the following is a balanced molecular equation describing the titration of a weak base and a strong acid?