answer with it either pH increase, pH decrease, no change, or cann't determine. a. What is the effect on pH that results from the addition NH4NO3 to NH3 solution? Use the equation below to answer the question: NH3 (aq) + H2O (l) ⇆ NH4+ (aq) + OH− (aq) b. Initially only 0.5 M HF solution is present: HF (aq) + H2O (l) ⇆ F− (aq) + H3O+ (aq). What happen if 0.5 mol of solid NaF is added to the initial HF solution? c. What is the effect on pH that results from the addition HCOONa to HCOOH solution? Use the equation below to answer the question: HCOOH (aq) + H2O (l) ⇆ HCOO− (aq) + H3O+ (aq)

Match each compound with the word or phrase that best describes it. Fe(OH)2 ✓HCIO ✓HSO4 ✓ HBr OH™ A. Strong electrolyte B. Arrhenius base C. proton acceptor D. Weak electrolyte E. Can behave as both an acid or a base

If there is a solution of weak acid (CH3COOH) and a solution of strong acid (HCl), what statement is true? 0.1 M 0.1 M HCI CH,COOH There are more H3O™ ions in the beaker with the strong acid There are more H3O™ ions in the beaker with the weak acid The amount of H3O™ ions will be the same in both beakers It is impossible to predict which beaker will have more H3O+

HCN(aq)+H2O(l) ⇄ H3O+(aq)+CN−(aq)               Ka=[H3O+][CN−] / [HCN]=6.2×10−10 The equilibrium reaction shown above represents the partial ionization of the weak acid HCN(aq). A 0.200M HCN(aq) solution has a pH≈4.95.   If 0.05g (0.010mol) of NaCN(s) is added to 100mL of 0.200M HCN(aq), which of the following explains how and why the pH of the solution changes?     a) The pH will be higher than 4.95 because adding CN− will disrupt the equilibrium, resulting in an increased production of HCN that decreases the concentration of H3O+.   b ) The pH will be lower than 4.95 because adding CN− will disrupt the equilibrium, resulting in an increased production of HCN that decreases the concentration of H3O+.   c)The pH will be higher than 4.95 because CN− is a strong base that can neutralize HCN.   d )The pH will remain close to 4.95 because the Ka is so small that hardly any products form.

Identify each of the substances in the reaction as acid, base, conjugate acid, or conjugate base. HSO, (aq) H¸O(1) 1, SO,² (aq) H,O*(aq) 31 --

3. Write equations for the formation of each salt. Write if the salt is,acidic, basic or neutral. Zn (aq) + HCL (D): (aq) ZnCl2 (aq) + H2 HCN__(aq) = NaCN (aq) + H₂O a) b) NaOH(aq) + c) (aq) + (aq) + (aq) + d) e) (aq) → CuSO4 (aq) + H2O (1): (aq) (NH4)2SO4 (aq) + (1): (aq) BaCl2 (aq) + (1):

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. C5H;NHI 2- + 2+ 3+ 4+ 1 2 3 4 6. 7 8 9 1 3 04 O6 O7 + (s) (1) (g) (aq) C OH H. NR H2O H30* N Reset • x H2O Delete LO 3.

Calculate the pH after adding 40.00mL of HCl. NH3 (aq) + HCl (aq) → NH4Cl (aq) 35mL of .1000M NH3 .1000M HCl

Part 1- What is the conjugate acid of H2PO4−? of NO3−? Part 2 -Write the balanced chemical equation for the neutralization reaction between Sr(OH)2 and H3PO4. What is the salt? Part 3 - If the concentration of H3O+ is 3.5 × 10-3 M, the concentration of OH−− is ________ M. (Show your Calculation) Part 4- Identify each substance as an Arrhenius acid, an Arrhenius base, or neither. b) HNO2 c) Ba(OH)2