When a redox reaction occurs in a basic solution the H+ needs to be neutralized.  In order to do this what needs to be added?

Which numbered response lists all of the following statements that are true and no false statements? A catalyst can…….. I. make a non-spontaneous reaction spontaneous II. speedup the forward reaction and slowdown the reverse reaction III. lower the activation energy of the forward reaction IV. lower the activation energy of the reverse reaction

A NaOH solution is to be standardized by titrating it against a known mass of potassium hydrogen phthalate (KHP). Which procedure will give a molarity of NaOH that is too low? 

Consider the following pairs of liquids. Which numbered response contains all the pairs that are miscible and non that are immiscible? I. Benzene (C6H6) and hexane (C6H14) II. Water (H2O) and methanol (CH3OH) III. Water (H2O) and hexane (C6H14)

The sum of 26.83 + 2.7120 + 7.15 + 138.12 + 150.2619 expressed to the proper number of significant figures is:

Consider the titrations of the pairs of aqueous acids and bases listed at the left. Which pair is incorrectly described (at the right) in terms of the acidic, basic or neutral character of the solutions ar the equivalence point?     Acid-Base Pair  Character at Equivalence Point  (A)    HClO + NaOH           acidic  (B)   HNO 3 + Ca(OH) 2           neutral  (C)  CH 3COOH  +  KOH           basic  (D)  HCl  +  NH 3           acidic  (E)  CH 3COOH  +  NH 3           neutral Hint: The conjugate base of a weak acid will hydrolyze water, similarly a conjugate acid of a weak base will hydrolyze water Example: HF + NaOH → H2O + F- + Na+; The F- is the conjugate base of the weak acid HF. The F- can react with water (hydrolysis) as shown below to produce OH- to make the equilibrium basic. F-  +  H2O  →  HF  +  OH-

In the following equation, CO is  Fe2O3(s)   +  3CO(g)  →  2Fe(s)  +  3CO2(g)

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. SO3 (g) + H2O (g) ↔ H2SO4 (l)                   ΔG O = -90.5 kJ P(SO3) = 0.20 atm; P(H2O) = 0.88 atm

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 OC. (The equation is balanced.)  Pb(s) + Br2 (l) à Pb2+ (aq) + 2 Br- (aq) Pb2+ (aq) + 2 e- à Pb (s)                  EO = -0.13 V Br2 (l) + 2 e- à2 Br- (aq)                  EO = +1.07 V

The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant. N2O4 (g) ⇌ 2NO2 (g)                 Kc = 1.46                                                      6NO2 (g) ⇌ 3 N2O4 (g)       Kc  = ?