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Acid-Base Chemistry
Page 7
Questions (825)
The triprotic acid H3A has ionization constants of Ka1 = 2.5× 10–4, Ka2 = 3.4× 10–8, and Ka3 = 5.4× 10–13. Calculate
1 answer
asked by
alex
992 views
What mass of ammonium chloride must be added to a 0.500 L solution of 0.250 M ammonia to make a buffer with a pH of 9.26? Kb
3 answers
asked by
paula
1,619 views
a solution containing 100.0 mL of 0.135 M CH3COOH (ka=1.8E-5) is being titrated with 0.54 M NaOH. calculate the ph:
at the
5 answers
asked by
jk
584 views
For a triprotic acid H2PO4. Ka1=7.11e-3, Ka2=6.32e-8 and Ka3=7.1e-13. 50mL each of 0.05F CaCl2 and 0.05F phosphoric acid were
6 answers
asked by
Mia
632 views
To have a buffer with a pH of 2.50, what volume of 0.510 M NaOH must be added to 100. mL of 0.230M H3PO4?
2 answers
asked by
Shannon
523 views
What is the ph of a .05 L solution containing .075 mol NH3 and 6.80 g of NH4+ when .025 L of 2 M is added to it? Kb= 1.8 x10^-5
4 answers
asked by
Lola
351 views
Calculate the pH of a solution made by adding 75.0 g of CH3COONa to 750 mL of 0.64 M
CH3COOH. Ka for CH3COOH is 1.8 x 10-5.
1 answer
asked by
nurul
446 views
Suppose you have added 200.0 mL of a solution containing 0.5000 moles of acetic acid per liter to 100.0 mL of 0.50000 M NaOH.
4 answers
asked by
Freddy
1,245 views
Determine the pH at the equivalence point in the titration of 41.0 mL 0.096 M formic acid with 0.108 M NaOH at 25oC.
Calculate
2 answers
asked by
Michelle
588 views
1)what is the final pH of CHECOOH 0.18M ,CHECOONa 0.08M, HNO3 0.08M and NaOH 0.08M ? Ka=1.8^10(-5)
2)what fraction of free edta
2 answers
asked by
airam
488 views
Should 25 ml of 0.15 M HCL solution be added to 250 mL of buffer solution containing 0.25M HF Ka-7.1 x 10, and 0.40 M NaF at a
1 answer
asked by
Always
380 views
d 25 ml of 0.15 M HCL solution be added to 250 mL of buffer solution containing 0.25M HF Ka-7.1 x 10, and 0.40 M NaF at a pH of
1 answer
asked by
Always
430 views
What happens if I try to make a pH 6 buffer by diluting 0.100 M HCL (aq) with water .
1 answer
asked by
debby
384 views
Alcohols are weaker acids then water,why ?
1 answer
asked by
Bharat
342 views
What is the pH of rainwater at 30C in which atmospheric Co2 has dissolved, producing a constant [H2Co3] of 1.40x10^-5 M? Take
2 answers
asked by
Monica
637 views
Calculate the pH of a solution prepared by adding 36 cm3 of 0.15 M methanoic acid to 27 cm3 of 0.20 M NaOH. (Ka for methanoic
1 answer
asked by
Teagan
358 views
What is the pH of a solution that contains 0.30 M HC2H3O2 and 0.95 M C2H3O2-? Use Ka = 1.8 × 10-5 for HC2H3O2.
2 answers
asked by
Dina
709 views
35.0mL sample of 0.150M acetic acid9HC2H3O2)(Ka=1.8*10-5) is titrated with 0.150M NaOH solution. calculate the pH AFTER 17.5 Ml
2 answers
asked by
mbuyelo
539 views
A student attempted to synthesize malonic acid which has a molecular weight of 104
g/mol by the same method used to synthesize
5 answers
asked by
Ana
950 views
What would the [OH-] be after addition of 17.47 mL of 0.1000 M NaOH to 25.00 mL of 0.1000 HA (a weak acid, Ka = 3.16e-4)?
1 answer
asked by
hershi
442 views
Calcualte PH and POh of an aqueous solution that is 0.050 M in HCL and 0.085 M in HBr at 25 degrees C
2 answers
asked by
Jason
891 views
A buffer solution is made by dissolving 0.45 moles of a weak acid (HA) and 0.23 moles of KOH into 680 mL of solution. What is
3 answers
asked by
gabriella
858 views
A 0.1 molar solution of nitrous acid is 7.1 percent ionised at equilibrium what is the
A. Concentration Hydrogen ion and ph B. Ka
2 answers
asked by
Rich addunya
106 views
Calculate the pH and include the balanced equation for the acid dissociation reaction.
0.20 M HC3H5O2 (propionic acid, Ka = 1.3 x
1 answer
asked by
<3
449 views
Calculate the pH of a buffer that is 0.250M in NaHCO3 and 0.300M in Na2CO3
2 answers
asked by
Anonymous
569 views
Calculate the pH at the equivalence point if 25.00 mL of 0.010M barbituric acid (HC4H3N2O3) is titrated with 0.020M NaOH. (Ka
2 answers
asked by
Mary
495 views
A 10.00 mL aliquot of a solution of a weak acid
, HA, whose pK a is 4.76 is titrated with OH - generated by electrolysis of water
1 answer
asked by
jody
377 views
Pls help..
Q: prepare a table of value for acid-base titration using 26.40cm^3 as end point
3 answers
asked by
Vivian
306 views
calculate the pH at 25 degrees of 0.080 mol dm^-3 HNO3
1 answer
asked by
roxanne
281 views
A sample of rain in an area with severe air pollution has a pH OF 3.5. What is the pOH of this rainwater?
4 answers
asked by
Lauren J.
892 views
How many milliliters of 0.202 M KOH should be added to 500.0 mL of 0.0233 M
tartaric acid (C4H6O6; FW 150.087) to adjust the pH
3 answers
asked by
Micki
514 views
what is the pka of cyclohexanaminium (C6H11NH3+)
3 answers
asked anonymously
18 views
a solution is made up of 0.001M dichloroacetic and 0.0001M acetic acid.find the pH using the charge balance
1 answer
asked by
tsogwane
934 views
Calculate the pH of 500. mL of 0.100 M acetic acid, CH3COOH, which also contains 0.100 mole of sodium acetate, NaCH3COO.
How do
1 answer
asked by
Bianca
764 views
calculate the pH pOH and (OH(aq)) of 0.006mol/l HI(aq)
2 answers
asked by
ashley
575 views
In the derivation of this expression:
[ln]/[HIn]A# 2 * A#1,acid/A# 2,basic * A#1 We assumed that the HIn form of the indicator
1 answer
asked by
Cristian
615 views
The pH of 0.02M solution of a weak acid was measured at 7.6. What is the [OH-] in this
solution? B) The Ka for benzoic acid is
2 answers
asked by
Emma
510 views
An unknown compound, X, is though to have a carboxyl group with a pKa of 2.0 and another ionizable group with a pKa between 5
2 answers
asked by
ron
896 views
How many milliliters of glacial acetic acid (17.3 M) would you need to titrate an aqueous solution of 100 grams sodium acetate
1 answer
asked by
Trey
407 views
The formula for determining the pH of a solution is pH = -log[H+], where [H+] is the hydrogen ion concentration (in M/L). What
2 answers
asked by
alejandro
506 views
What is the pH of a .20M HA solution (Ka=1.0x10^-6) that contains a 0.40M NaA?
3 answers
asked by
Liz
607 views
Enough of a monoprotic acid is dissolved in water to produce a 0.0165 M solution. The pH of the resulting solution is 2.38.
4 answers
asked by
RZeal
1,743 views
Calculate the pH of a 75.0 ml solution containing 0.85 M lactic acid after the addition of 0.0225 moles NaL (assume a negligible
7 answers
asked by
Davis
466 views
What is the pH of 0.144M aqueous solution of ammonium nitrate?
I am not sure what to do. Would I do 10^-0.144^ = 0.71?
7 answers
asked by
Hannah
356 views
How would an HA acid behave in water if it were a strong acid, weak acid, and non-electrolyte?
1 answer
asked by
Robert
427 views
What is the [H3O+] for a neutral solution at 50 degrees celsius?
I know that kw=[H3O+][OH-] but I am not sure what to do to get
4 answers
asked by
Hannah
1,146 views
A solution is prepared by mixing 499 mL of 0.19 M Tris·Base and 592 mL of 0.37 M Tris·Acid. What is the pH of this solution?
2 answers
asked by
Brittany
476 views
1) The approximate pH of a 3.0 X 10^-3 M solution of the strong acid H2SO4 is?
I did pH= -log(3.0 X 10^-3) = 2.5 2)If HCLO2 is a
3 answers
asked by
Hannah
529 views
Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.0
2 answers
asked by
Frank
735 views
one last question DrBob222 U wrote:
I did not guess. You said a weak acid and NaOH so I picked acetic acid (which I will call
3 answers
asked by
HELP PLEASE to DrBob222
448 views
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