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Acid-Base Equilibrium
Page 3
Questions (295)
Find the pH of mixture of acids. 0.185 M in HCHO2 and 0.225 M in HC2H3O2
Im using an ice chart of weak acid and putting in strong
4 answers
asked by
L.Bianchessi
4,102 views
calculate the hydronium ion concentration in 0.125M formic acid, HCHO2
Ka= 1.8 x 10-4 can you show me the steps pls
6 answers
asked by
Monique
1,082 views
The Ka value of nitrous acid, HNO2 , is 4.0 × 10¯4 . What is the equilibrium constant for the reaction; NO2¯ + H2O <-> HNO2 +
4 answers
asked by
Thomas
890 views
How many grams of NaOH(Mr 40) must be added to 100 ml of 0.1M H3PO4 to create phosphate buffer, pH 7.0?
I know I'm using
4 answers
asked by
Dilk
682 views
For a solution that is 0.20 M HCN(aq) with a Ka=4.9x10^-10
a. calculate the [H+] b. calculate the [OH-] c. what's the pH? Please
4 answers
asked by
Sharon
2,453 views
What is the value of [OH-] in a 0.015 M CH3COOH solution? Ka = 1.8 x 10-5
I started by writing the equation: CH3COOH + H2O <--->
3 answers
asked by
Audrey
930 views
Given that Kw = 2.4x10^-14 at 37 celsius, compute the PH of a neutral aqueous solution at 37 celsius, which is the normal human
3 answers
asked by
Kim
869 views
Calculate the [NH4+] in solution that is 0.25 M NH3 and 0.20 M NaOH. (Kb for NH3 = 1.8 x 10-5)
I set up ICE from the equation:
4 answers
asked by
AMI
1,480 views
For the reaction of hydrazine (N2H4) in water, Kb is 3.0 10-6.
H2NNH2(aq) + H2O(l) H2NNH3+(aq) + OH -(aq) Calculate the
3 answers
asked by
Lori
1,461 views
A buffer solution is composed of 1.00 mol of acid and 3.25 mol of the conjugate base. If the pKa of the acid is 5.00, what is
2 answers
asked by
paige
25 views
You are asked to bring the pH of 0.500 L of 0.450 M NH4Cl to 7.00.
12.0 M NH3 How many drops (1 drop 0.05 mL) of this solution
2 answers
asked by
K
696 views
Calculate [H3O+]
0.100 M NaNO2 and 5.00×10−2 M HNO2 so there's no Ka value for NaNO2, it can be ignored 5.6x10^-4 = x^2 /
2 answers
asked by
X
927 views
This is regarding the Biochemistry question postef by Grace..
I'm wasn't able to mention this in the subject section due to the
3 answers
asked by
Shenaya
459 views
Calculate the relative concentration of phenol (ka=1.05x10^10) and phenolate ion in a solution with 0.05M total phenol (pH=7.5)
3 answers
asked by
Siobhan
884 views
What is the pH of 1.00 L of the 0.100 M hydrofluoric acid/0.120 M fluoride ion buffer system from the previous problem after
1 answer
asked by
kinks
360 views
The [OH-] ion concentration of a sample is 1 × 10-10 M. What is the concentration of [H+] in the sample at 25°C?
A. 1 × 10-14
3 answers
asked by
erika
628 views
How can we calculate the HCO3- (bicarbonate ion) concentration in water in 25C pH7.0?
I think we can use PV=nRT equation, but I
1 answer
asked by
Anonymous
459 views
calculate the concentration of acetic acid in a 0.85 m sodium acetate solution,when ph=7,knowing that for the acetic acid,ka=
1 answer
asked by
Anonymous
380 views
Check my work?
What is the approximate pH of a 0.05 M solution of HSCN that has a Ka of 10-4? HSCN -> H+ + SCN-
4 answers
asked by
Aurora
1,245 views
For the diprotic weak acid H2A, Ka1 = 2.0 × 10^-6 and Ka2 = 6.7 × 10^-9.
What is the pH of a 0.0800 M solution of H2A? What are
2 answers
asked by
GARRETT
934 views
a buffer solution is 0.2M in acetic acid and in sodium acetate. Calculate the change in pH upon adding 1.0ml of 0.1M
2 answers
asked by
woo
725 views
Please help with the solution:
Question asks: A solution has [OH-] = 2.0 X 10 negative ^14. The [H-] in this solution is 2.0 x 10
1 answer
asked by
Cassandra
321 views
Alright, this time, I know I have not mistyped my answer.
Find the initial concentration of the weak acid or base in an aqueous
3 answers
asked by
Ethan
481 views
Calculate the concentration of H3O
+ present in 0.377 M H2CO3. Answer in units of mol/L I know the Ka of H2CO3 is 4.3E-7. But I
5 answers
asked by
Ethan
744 views
Butanoic acid (Ka = 1.52 x 10-5) has a partition coefficient of 3.0 (favouring benzene) when
distributed between water and
2 answers
asked by
Daniel
1,067 views
using Kb, for NH3 (from Appendix E), calculate Ka for the NH4+ ion.
Kb for NH3 is 1.81 x 10^-5 Ka for NH4+ is Kw / Kb = 10^-14 /
2 answers
asked by
Tim
1,315 views
a) Write Bronsted acid-base equilibrium equations for the following:
b) Show the acid-base conjugated species, labeling all
2 answers
asked by
Sean
513 views
It was determined that a 0.10 M solution of an acid was only 2.5% ionkzed. Find the Ka and pKa for the acid.
3 answers
asked by
Jordan
282 views
How to start these problems out: Please help thank you
Use the Henderson-Hasselbach equation: pH = pKa + log [A-]/[AH], where A-
10 answers
asked by
meghan
537 views
use the dissociation constant ka=[H+][A-]/[HA] to show that ph=pka
1 answer
asked by
jewels
363 views
an acid with the equilibrium concentration is listed below:
1) HA + H2O = H3O^+ + A- HA= 10^-1 M, H3O=10^-3M, A=10^-3M Calculate
2 answers
asked by
Hannah
544 views
50.0mL of 0.1 molar NaOH is added with 50.0mL of 0.1 molar CH3COOH. The Ka = 1.8*10^-5. what is the pH of the solution?
a) 7.00
1 answer
asked by
Zac
422 views
Tris is an abbreviation for tris (hydroxymethyl) aminomethane, which is a weak base. Calculate how many grams of tris
4 answers
asked by
Cassandra
1,181 views
1) The Ka for acetic acid is 1.8e-5. What is the pH of a 3.18M solution of this acid?
I did 1.8e-5 = x^2/3.18 x=sqrt 1.8e-5 X
6 answers
asked by
Hannah
401 views
calculate the pH when 10 mL of .511 M sodium acetate and 20.00 mL of 0.350 M acetic acid
1 answer
asked by
brooke
277 views
What would happen to a weak base dissociation equilibrium if more products were added?
2 answers
asked by
princess
853 views
which of the following has the highest bugger capacity?
A 0.10M H2PO4-/0.10M HPO4 -2 B 0.50 M H2PO4-/0.10 M HPO 2- C 0.10 M
2 answers
asked by
ameryss
580 views
1)calculate [OH-] and pH for each of the following solutions. (Kw = 1.0*10^-14.)
a)0.101 M NaF b) 0.030 M Na2S c)a mixture that
2 answers
asked by
MARY
619 views
A) Calculate [OH^-] in a o.12 M solution of hydrazine, H2NNH2(aq), having K of 3.0x10^-6.
B) what is the percent ionization of
4 answers
asked by
Jacob
725 views
Calculate the pH of 0.0115M acetic acid solution at 25 degrees celcius with Ka = 1.75*10^-5
1 answer
asked by
Gift
469 views
So I've been working on this online homework problem and got it wrong 8 times. I need help. Here's the question:
1,2-diaminoethan
1 answer
asked by
Dre
1,041 views
2.50 mL of ethyl acetate and 2.50 mL of distilled water are added to the 5.00 mL of 3 Molar HCl and the mixture is allowed to
2 answers
asked by
Tichele
561 views
What is the new pH when 1mL of 1M HCl os added to 5mL of 0.1M Phosphate buffer (pH 7.4)?
2 answers
asked by
Rose
640 views
Calculate the [CH3NH3+] of a 7.02×10-3 M solution of the weak base CH3NH2 (make an approximate calculation assuming that
2 answers
asked by
sparkle
557 views
Suppose that 55 mL of 0.2 M LiOH and 55 mL of 0.3 M HNO2 are mixed.
What is the K for the dominant equilibrium in terms of Ka's,
1 answer
asked by
Tiffany
446 views
Calculate the [H3O+] of each aqueous solution with the following [OH-]:
urine, 1.8 x 10^-9 M Express your answer to two
3 answers
asked anonymously
33 views
0.10 moles HCOOH (formic acid) and 0.02 moles HCOONa (sodium formate) are dissolved in a liter of water. what is the resulting
1 answer
asked by
Anonymous
518 views
You have to design a buffer based on one of the systems below
System 1: HA1 and A1-1 K= 4 E-3 System 2: HA2 and A2-1 K= 5 E-4
1 answer
asked by
maya
442 views
Hi again!
I have a new question, Can you help me? Consider 50.0 mL of a solution of a weak acid HA (Ka = 1.00.E-6), which has a
1 answer
asked by
Mary
366 views
(a) Find pH and pOH of 1.0 M solution of sodium benzoate, NaC6H5COO. (Ka of benzoic acid is 6.2x10^-5)
(b) Calculate pH after
7 answers
asked by
Marissa
2,061 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
Solutions
Solutions and Acids/Bases
Solutions and Concentrations
Solutions and Equilibrium
Stoichiometry
Thermodynamics