Complete a net ionic equation for each proton-transfer reaction. NH4* + OH - Draw the formulas of the two products. • Draw cations and anions in separate sketchers. Separate structures with + signs from the drop-down menu. ● 0- 90-85 soll H-N H CH3 ChemDoodle Sn [F +v D 0- ▾ **** E H-O-H
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- Dilution is necessary for commercially available acids such as HNO3, H2SO4 etc so that the strength is increased so that students use it conveniently in a chemistry laboratory. Select one: True O FalseComplete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO3(aq) > 4- 3. 2+ 3+ 4+ 1 2 6 7 8 O2 4 5. ) (s) (1) (g) (aq) H N H30* CI H20 OH 4- +Is H2Cr2O2 an acid, base, or neutral? please justify your answer with an equation showing its dissociation.
- Draw a structure for the product of the acid-base reaction below. t H3C CH3 . Include all valence lone pairs in your answer. • If the reaction is a Lewis acid-base reaction, draw the products in a single sketcher, with a single bond connecting the Lewis base and Lewis acid. • If the reaction is a Brønsted acid-base reaction, draw the products in separate sketchers. • Include all nonzero formal charges. 3 TI +▾ + AICI 3 *9-85 CH To Q Q 4 [F Previous3. 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.Complete the table. (The first row is completed for you.) Acidic or (H30*] (OH] pOH pH Basic 1.0 x 10-8 1.0 x 10-6 6.00 8.00 basic 3.55 1.7 x 10-9 13.5 8.6 x 10-11 ||
- 7b. What is the strongest intermolecular interaction that would occur between a molecule of NH3 with a molecule of SbH3? 7c-d. In aqueous solution, NH3 (aq) acts as a weak base. 7c. When NH3 is added to otherwise pure water, we would expect: (circle answers) The concentration of OH- (aq) to: (i) increase (ii) decrease (iii) stay the same The pH to: (i) increase (ii) decrease (iii) stay the sameCalculate the H*| and pH of a 3.05 × 10–4 M nitrous acid solution. The Ka of nitrous acid is 7.10 × 10–5. [H*] = M pHWrite the net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium nitrate is dissolved in water. (Use H;O* instead ofH".) + H,O(1) This solution is +
- Reaction 1: NaOH(s) -> Na+(AQ) + OH-(AQ) Reaction two: Na+(AQ) + OH-(AQ) + H+(AQ) + -> H2O(I) + Na+(AQ) Assuming reaction 1 has a enthalpy of 59.12 KJ/mol and reaction 2 has a enthalpy of 46.06 kJ/mol Calculate the change in enthalpy for the reaction shown below NaOH(s) + H+(aq) -> H2O(I) + Na+(aq) Delta H = ?Interpret the following reactions in terms of Lewis theory: a) CH3I + OH - ↔ CH3OH + I - b) Cu+2 + 4NH3+(aq) ↔ Cu(NH3)4+2(aq) c) C2H3O2- + H+ ↔ HC2H3O29) a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; + H;O* H¿CO; + H2O (aqueous solution) b) Phenol (HC&H50) is a weak acid (Ka= 1.5 x 10*). Write the equilibrium chemical equation, equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol. 10) Blood is mainly buffered by HCO; /H2CO; (H2CO3, Carbonic Acid, K= 4.4x10 -") buffer system. Calculate the pH of human blood for a carbonic acid concentration of 0.091M and HCO; concentration of 1.00M.