0
answers
0
watching
161
views
11 Dec 2019
1. A 0.100 m solutuon of bromoacetic acid (BrCH2COOH)is 13.2% ionized. Calculate [H+],[BrCH2COOH]and Ka for bromoacetic acid.
2. Complete and balance the following equations, and identiy theoxidizing and reducing agents. (Recall that the O atoms in hydrogenperoxide, H2O2 have an atypical oxidationstate.)
a) NO2-(aq) +Cr2O72-(aq) -->Cr3+(aq) + NO3-(aq) (acidicsolution
b) S(s) + HNO3(aq) -->H2SO3(aq) + N2O(g) (acidicsolution)
c)Cr2O72-(aq) +CH3OH (aq) --> HCO2H (aq) +Cr3+(aq) = acidic solution)
d) BrO3-(aq)+N2H4(g) --> Br- (aq0 +N2 (g) (acidic solution)
e) NO2-(aq) + Al(s) -->NH4+(aq) + AlO2-(aq)(basic solution)
f) H2O2(aq) + ClO2(aq)-->ClO2-(aq) + O2(g) (basicsolution)
1. A 0.100 m solutuon of bromoacetic acid (BrCH2COOH)is 13.2% ionized. Calculate [H+],[BrCH2COOH]and Ka for bromoacetic acid.
2. Complete and balance the following equations, and identiy theoxidizing and reducing agents. (Recall that the O atoms in hydrogenperoxide, H2O2 have an atypical oxidationstate.)
a) NO2-(aq) +Cr2O72-(aq) -->Cr3+(aq) + NO3-(aq) (acidicsolution
b) S(s) + HNO3(aq) -->H2SO3(aq) + N2O(g) (acidicsolution)
c)Cr2O72-(aq) +CH3OH (aq) --> HCO2H (aq) +Cr3+(aq) = acidic solution)
d) BrO3-(aq)+N2H4(g) --> Br- (aq0 +N2 (g) (acidic solution)
e) NO2-(aq) + Al(s) -->NH4+(aq) + AlO2-(aq)(basic solution)
f) H2O2(aq) + ClO2(aq)-->ClO2-(aq) + O2(g) (basicsolution)