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Acid-Base Equilibrium
Page 2
Questions (295)
The total phosphate concentration in a blood sample is determined by spectrophotometry to be 3.0×10−3 M. The pH of the blood
4 answers
asked by
India
1,932 views
calculate the hydronium ion concentration in an aqueous solution that contains 2.50x10^-6M in hydroxide solution
4 answers
asked by
brittney
5,407 views
For my lab, I have been asked to calculate the pKa of an unknown amino acid. We titrated the unknown amino acid with NaOH. The
4 answers
asked by
Eleanor
1,170 views
Mg(OH)2(aq) <--> Mg2+ (aq) + 2OH-(aq)
a) what would happen to the equilibrium if some acid is added to the soultuion? b) what
4 answers
asked by
Zander
1,736 views
The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 x 10-5) and 0.172 M sodium acetate is
__________. The Ka of
5 answers
asked by
jack
3,338 views
The Ka of HClO is 3.0x 10^-8 at 25°c. What is the percent ionization of HClO in a 0.015M aqueous solution of HCLO at 25°c?
4 answers
asked by
Zekariyas
1,588 views
Calculate the concentrations of all species present in a 0.100 M solution of weak polyprotic acid H3PO4. Ka1=7.5 x 10 ^-3, ka2 =
6 answers
asked by
Kate
2,313 views
Calculate the concentrations of all species in a 0.690 M Na2SO3 (sodium sulfite) solution. The ionization constants for
3 answers
asked by
Jack
2,303 views
1)What is the pH of a 0.25 M solution of acetate (CH3COO-) with a pKa of 4.76?
2)If the [OH] of a solution is 2.95 x 10-5M, what
4 answers
asked by
ChemEmergency
1,473 views
A biochemist prepares a lactic acid-lactate buffer by mixing 225 mL of 0.85M lactic acid with a Ka=1.38*10^-4 with 435mL of
4 answers
asked by
Mike
3,038 views
A 0.040M solution of a monoprotic acid is 14% ionized. Calculate the Ka for the weak acid.
---------------- so: HX <---> H+ + X-
3 answers
asked by
Saira
2,888 views
A 0.035 M solution of a weak acid (HA) has a pH of 4.88. What is the Ka of the acid?
HA ==>H^+ + A^- Ka = (H^+)(A^-)/(HA) pH =
3 answers
asked by
Paul
1,673 views
Calculate the hydronium ion concentration of a 0.250M solution of ethaonic acid (Ka= 1.82 x 10^-5)
5 answers
asked by
Abednego Kumye
1,253 views
The pKb of ammonia, NH3, is 4.74 at 25°C. Which of the following is the Ka of the ammonium ion, NH4+?
not sure what to do,
4 answers
asked by
chem101
1,873 views
What is Kc for the following equilibrium? For phosphoric acid, Ka1=6.9x10^-3, Ka2=6.2x10^-8 and Ka3=4.8x10^-13
HPO4^-2 + OH^-
6 answers
asked by
Sara
1,038 views
If you have 0.2 M of NaC7H4ClO2 with a pH of 8.65, what is the pH of 0.2 M of HC7H4ClO2?
4 answers
asked by
Allison
629 views
Calculate the pH of (a) a solution that contains 0.10 M HNO3(aq) (Ka ~20 M) and 0.10 M HCN(aq) (Ka = 6.2 × 10–10 M), (b) a
3 answers
asked by
need help
699 views
Use the henderson-hasselbalch equation to predict the change in pH when 0.50ml of 1M HCl is added to 40mL of .10M buffer at pH 6
11 answers
asked by
Heidi
811 views
What are the equilibrium concentrations of H2SO3, H+, HSO3−, and SO32−in a 0.050 M solution of sulfurous acid H2SO3 at 25
3 answers
asked by
ston
1,599 views
Calculate pH of 0.01 M CH3COONa solution if pKa of CH3COOH is 4.74.
4 answers
asked by
kartikaya
3,148 views
Calculate [H3O+] and [OH-] in 0.22M KOH(aq)
3 answers
asked by
Shellu
1,039 views
How do I predict whether the equilibrium lies to the right or left of an Acid-base equation?
O[2-](aq) + H2O(l) <--> OH[-] +
3 answers
asked by
Ana
1,618 views
what is the pH of a solution that is 0.200 M in methylamine, CH3 NH2
CH3NH2+ H20<======> CH3NH3+ + OH- Kb= 4.2 x 10 ^-4
4 answers
asked by
shanice
1,516 views
The S^2- ion is a relatively strong base with an equilibrium constant of 7.7x10^-1.
What is the Ka value for HS- ? I got the
5 answers
asked by
sh
886 views
0.10 M methylamine (CH3NH2)
kb= 4.38e-4 calc the percent ionization so i did the ICE table to find that x=6.26e-3 and then i
4 answers
asked by
Spencer
3,363 views
Caclulate the Ka of nitrous acid if a 0.200 mol/L solution at equilibrium at SATP has a percent ionization of 5.8%
ka=(H+)(NO2-)/
4 answers
asked by
Dustin
1,081 views
Calculate the hydronium ion concentration in 50.0 mL of 0.10M NaH2AsO4.
and we are given K1 = 6.0E-3, K2 = 1.1E-7 and K3 =
3 answers
asked by
Vic
998 views
What are the equilibrium concentrations of all the solute species in a 0.95 M solution of hydrogen cyanide, HCN? The Ka value =
3 answers
asked by
Alice
1,016 views
If a solution of NaOH is left exposed to room air, what will happen to its pH? What chemical
equilibrium is responsible for this
4 answers
asked by
Leul
538 views
The weak acid HQ has pKa of 4.89. Calculate the (OH-) of 0.500 M HQ
This is what I have: pKa = 4.89 so Ka = 10^-4.89 = 1.29x10^-5
3 answers
asked by
patrick
825 views
Which of the following equations correspond to the Ka2 for phosphoric acid?
note: the double equal sign (==) means equilibrium.
3 answers
asked by
Hannah
1,960 views
ph at equivalence point when 25 ml of a 0.175M solution of acetic acid is titrated with 0.10M of NaOH at its end point
3 answers
asked by
Sharnam
562 views
A buffer, consisting of H2PO4− and HPO42−, helps control the pH of physiological fluids. Many carbonated soft drinks also
3 answers
asked by
HELP PLEASE
841 views
Calculate [CO32- ] in a 0.019 M solution of CO2 in water (H2CO3). If all the CO32- in this solution comes from the reaction
3 answers
asked by
Kaleen
1,953 views
calculate the pH of a buffer solution containing 0.200M acetic acid, HC2H3O2, plus 0.150M sodium acetate. The dissociation
12 answers
asked by
Monique
1,826 views
what is the equilibrium concentration of acetate ion if the equilibrium concentration of acetic acid is .40 M, the pH is 3.85,
3 answers
asked by
Anna
1,087 views
What is Ka for 4-aminobenzoic acid if a 0.020 M solution of the acid has a pH of 3.31?
a. 2.5 ´ 10-2 b. 2.0 ´ 10-2 c. 4.9 ´
3 answers
asked by
james
513 views
What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.74 at equilibrium? ka =1.7x10^-4
3 answers
asked by
rodrigue
917 views
what will be the pH of a 100mL buffer solution containing 0.064 M of acetic acid and 0.036M f sodium acetate, after addition of
4 answers
asked by
lia
555 views
Calculate the relative concentrations of phenol (Ka = 1.05 x 10-10) and phenolate
ion in a solution with 0.05 M total phenol (pH
4 answers
asked by
Anonymous
449 views
Now use the average value of Kb the base dissociation constant of acetate anion to calculate an average value for Ka, the acid
3 answers
asked by
Jenn
3,098 views
a solution contains 0.216 moles of a base and 0.614 moles of the conjuagte acid in a total volume of 800 mL. The pH of the
6 answers
asked by
JH
660 views
What is the concentration of arsenate ions in 3.5 M solution of arsenic acid?
The acid-dissociation constants of H3AsO4 are: Ka1
3 answers
asked by
Kelly
681 views
Given the molar concentration of hydrogen ion, calculate the concentration of hydroxide ion [H+]=7.9*10-7
3 answers
asked by
Anonymous
1,019 views
what is the hydronium ion concentration of a 0.35M oxalic acid, H2C2O4. solution? for oxalic acid, ka1= 5.6x10^-2 and
4 answers
asked by
Anonymous
1,777 views
calculate the kb of ammonia if the ph of .5M solution is 11.48
3 answers
asked by
Serge
798 views
The pH of a .10M HOBr solution is 4.8
1. What is [H+] in that solution? 2. What is [OBr-]? What is [HOBr]? (where do the H+ and
3 answers
asked by
Ray
2,370 views
what is the pOH of a 0.12 M solution of pyridine (Kb=1.4x10^-9) at 25 Celsius
3 answers
asked by
C
605 views
What are the equilibrium concentrations of H2SO3, H+, HSO3−, and SO32−in a 0.050 M solution of sulfurous acid H2SO3 at 25
2 answers
asked by
ston
918 views
Calculate the pH of an aqueous solution containing 3.8 10-2 M HCl, 1.0 10-2 M H2SO4, and 3.3 10-2 M HCN.
3 answers
asked by
Ashley
396 views
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Parent Categories (28)
Acids and Bases
Aqueous Solutions
Biochemistry
Chemical Equations
Chemical Equations Balancing
Chemical Equilibrium
Chemical Reactions
Chemical Reactions and Equilibrium
Chemical Reactions/Equilibrium
Chemical Solutions
Chemistry
Equilibrium
Equilibrium Chemistry
Equilibrium Constants
Equilibrium Reactions
Organic Chemistry
Physical Chemistry
Reaction Equations
Solution
Solution Calculations
Solution Chemistry
Solution Concentration
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Solutions and Acids/Bases
Solutions and Concentrations
Solutions and Equilibrium
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