Question
In: Chemistry
Consider the titration of 42.8 mLmL of 0.265 MM HFHF with 0.185 MM NaOHNaOH. Calculate the...
Consider the titration of 42.8 mLmL of 0.265 MM HFHF with 0.185 MM NaOHNaOH. Calculate the pHpH at each of the following points.
Part A
How many milliliters of base are required to reach the equivalence point?
Express your answer using three significant figures.
Part B
Calculate the pHpH after the addition of 10.7 mLmL of base
Express your answer using two decimal places.
Part C
Calculate the pHpH at halfway to the equivalence point.
Express your answer using two decimal places.
Part D
Calculate the pHpH at the equivalence point.
Express your answer using two decimal places.
Part E
Calculate the pHpH after the addition of 85.6 mLmL of base.
Express your answer using two decimal places.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A. A 75.0-mLmL volume of 0.200 MM NH3NH3 (Kb=1.8×10−5Kb=1.8×10−5) is titrated with 0.500 MM HNO3HNO3. Calculate...
A. A 75.0-mLmL volume of 0.200 MM NH3NH3
(Kb=1.8×10−5Kb=1.8×10−5) is titrated with 0.500 MM HNO3HNO3.
Calculate the pHpH after the addition of 11.0 mLmL of HNO3HNO3.
B. A 50.0-mLmL volume of 0.15 MM HBrHBr is titrated with 0.25 MM
KOHKOH. Calculate the pHpH after the addition of 15.0 mLmL of
KOHKOH.
C. A 52.0-mLmL volume of 0.35 MM CH3COOHCH3COOH
(Ka=1.8×10−5Ka=1.8×10−5) is titrated with 0.40 MM NaOHNaOH.
Calculate the pHpH after the addition of 17.0 mLmL of NaOHNaOH.
Consider a grating with 84 lines/mm and 15 mm of illuminated area. Calculate the wavelengths of...
Consider a grating with 84 lines/mm and 15 mm of illuminated
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Calculate the pH of 100.0 mL of a buffer that is 0.0650 M NH4Cl and 0.185...
Calculate the pH of 100.0 mL of a buffer that is 0.0650 M NH4Cl
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HNO3.
Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl and 0.185...
Calculate the pH of 100.0 mL of a buffer that is 0.060 M NH4Cl
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Consider the titration of 0.050 M HCl with 0.050 M NaOH. Calculate the pH: (a) of...
Consider the titration of 0.050 M HCl with 0.050 M NaOH.
Calculate the pH: (a) of the pure HCl solution; (b) of 25.00 mL
acid plus 12.50 mL base; (c) at the quivalence point; and (d) of
25.00 mL acid and 37.50 mL base.
A. Calculate the hydronium ion concentration in an aqueous solution of 0.185 M carbonic acid, H2CO3...
A. Calculate the hydronium ion concentration in an aqueous
solution of 0.185 M carbonic
acid, H2CO3
(aq)
B. Calculate the concentration of
HCO3- in an aqueous solution
of 0.1860 M carbonic acid,
H2CO3 (aq).
Consider a 9 mm diameter circular tube, calculate the length of tube that is required to...
Consider a 9 mm diameter circular tube, calculate the length of tube that is required to transfer 100 W of
water that circulates through the tube at a rate of 0.08 kg / s.
The temperature of the water is kept constant at 50 ° C and the wall
of the tube is maintained at 45 ° C.
Consider the titration of 42 mL of 0.111 MNaOH with 0.0803 MHCl. Calculate the pH after...
Consider the titration of 42 mL of 0.111 MNaOH with 0.0803 MHCl.
Calculate the pH after the addition of each of the following
volumes of acid. 6.8mL, 42mL, .10L
Consider the titration of 42.5 mL of 0.215 M HClO4 with 0.124 M KOH. Calculate the...
Consider the titration of 42.5 mL of 0.215 M HClO4 with 0.124 M
KOH. Calculate the pH of the resulting solution after the following
volumes of KOH have been added. (Assume that all solutions are at
25°C.) (a) 0.0 mL WebAssign will check your answer for the correct
number of significant figures. (b) 10.0 mL WebAssign will check
your answer for the correct number of significant figures. (c) 40.0
mL WebAssign will check your answer for the correct number of...
Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the...
Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121
M NaOH. Calculate the milliliters of base that must be added to
reach the first, second, and third equivalence points.
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