Questions LLC
Login
or
Sign Up
Ask a New Question
Acid-Base Chemistry
Page 9
Questions (831)
Hydronium ions are composed of
OH- H+ H2O Which one
1 answer
asked by
michael
346 views
if hydrogen flouride (HF) is dissolved in pure water will the pH of the solution be lesser or greater than 7? please explain
3 answers
asked by
heather
486 views
Can someone please help me and let me know if these questions and answers are correct? I just need a second opinion…and if
2 answers
asked by
Jess
773 views
(1) A beaker with 165 mL of an acetic acid buffer with a pH of 5.00 is sitting on a bench top. The total molarity of the acid
3 answers
asked by
Ashley
1,086 views
Known:
Cyanaocetic acid Ka=3.55*10^-3 ionization equation: HC3H2NO2<==> H^+ + C3H2NO2^- Unknown: pH of 0.4M of Cyanaocetic acid
1 answer
asked by
anonymous
435 views
How do you calculate the pH when the following substances are added to a buffer.(all of the solutions are at .10M conc.)
The
2 answers
asked by
Mary
572 views
Question..
Nicotinic acid (niacin) is a monoprotic acid with the formula HC6H4NO2. A solution that is 0.012M in the nicotinic
4 answers
asked by
Rushi
690 views
Posted by Kat on Monday, March 2, 2009 at 11:21am.
A solution of volume 80.0 mL contains 16.0 mmol HCHO2 and 9.00 mmol NaCHO2. If
4 answers
asked by
Kat
556 views
Calculate the ph of a 0.20 M solution of NH2BR
1 answer
asked by
MMmm
1,012 views
Assuming pKa values of 3.8 for the a-COOH and 8.5 for the a-amino groups and that the numbers in parentheses indicate the pKa
1 answer
asked by
Andrew
479 views
Find the net charge of cysteine at pH 8.75 using the follwing pka values:
carboxyl group has pka=1.9 amino group pka= 10.7 side
1 answer
asked by
Stephanie
533 views
Calculate the pH of concentrated hydrochloric acid if this solution is 24.8 % HCl by weight and has a density of 1.16 g/mL.
a. )
1 answer
asked by
A.A
471 views
Hi could someone please help me in the next 5 minutes with this question:
Given this data: mass of unknown acid 1.4671g Volume of
1 answer
asked by
janet
621 views
What is the pH of the solution created by combining 11.10 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)?
This is
5 answers
asked by
Amy
637 views
What would be the pH of a mixture of 50.0 mL of 0.0614 M HI and 75.0 Ml of 0.0845 M NH4NO3??
When i worked this question out, i
4 answers
asked by
Katie L
482 views
does the addition of a strong acid increase the percent ionization of a weak acid HB?
2 answers
asked by
blair
659 views
What is the pH of a 0.570 M solution of aniline? Kb = 7.4 × 10-10
3 answers
asked by
nelson
1,640 views
A) If you make up a solution of 50 mL of 0.1 M TRIS in the acid form, what will be the pH?
B) If you add 2 mL of 1M NaOH to the
1 answer
asked by
erin
1,126 views
Acid base Chenistry Homework help!?
Histidine was electrophoresed in polyacrylamide at pH 6.0 with alanine (pI=6.0) and arginine
1 answer
asked by
Mae
401 views
"experiment: spectrophotometric determination of the acid dissociation constant of methyl red"
1. Why is pH plotted against
1 answer
asked by
smiley
432 views
calculate the pOH of 3X106-6M of HF
1 answer
asked by
CHEM
351 views
Show that for the titration of a weak acid, HA, with NaOH solution, at half-titer, pH = pKa.
Please explain your answer. Thank
1 answer
asked by
phil
504 views
A 0.15 M solution of butanoic acid, C3H7COOH, has a pH of 2.8210. Find the Ka of butanoic acid.
Call buanoic acid HB. Then the
1 answer
asked by
Jess
1,267 views
I was absent for this info and im stuck.
A)calculate the pH in an acid-base titration when 10.00mL o 1.000 m NaOH is added to
1 answer
asked by
Just
441 views
WHAT IS PK2?
pK2 for H3PO4. Look in your text for k2 for H3PO4. My text, but it's an OLD OLD one lists k2 of 6.2E-8 and pK2 =
1 answer
asked by
Delli
416 views
i posted this question previously and got help however im still having some confusion. can u clarify ?
what's the pH of the acid
1 answer
asked by
Christine
448 views
Sulfuric Acid (H2SO4) is a strong acid, which dissociates when dissolved in water according to the following equation:
H20SO4(aq)
1 answer
asked by
Adam
727 views
I understand that the pH at the half equivalence point gives is the pKa value but could someone explain why this point is the
1 answer
asked by
amy
477 views
Alright, here is my question:
22. References list the Ka value of hydrosulphuric acid, H 2S(aq) , as 1.1 x 10^–7 at 25°C.
1 answer
asked by
Jacy
521 views
Which of the following is considered acidic?(1 point)
Responses Ammonia Ammonia Lime Water Lime Water Soap Soap Vinegar
1 answer
asked anonymously
35 views
How do phenolphthalein, bromothymol and methyl orange behave in acid base titration
1 answer
asked by
Kelvin
51 views
A buffer is made by dissolving H3PO4 and NaH2PO4 in water. a. write an equation that shows how this buffer neutralizes a small
4 answers
asked by
marcy
5,269 views
Why is AlCl3 an Arrhenius Acid, while BCl3 is not?
How can I determine which is an Arrhenius Acid?
3 answers
asked by
Jematormal91
3,759 views
what is the conjugate base of H2SO3??
3 answers
asked by
Anonymous
3,003 views
How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the
3 answers
asked by
Victoria
2,880 views
Calculate the pH of (1)0.150M KC2H3O2:
(2)0.200M pyridine chloride, C5H5NHCl: and(3) 0.500M NaCl
3 answers
asked by
Joshua
2,764 views
What would be the pH of a 0.1 M aqueous solution of the phenolate ion, C6H5O–? (Ka for phenol, C6H5OH, is 1.3 x 10–10) I got
4 answers
asked by
Nat
2,333 views
The pH of a 0.25 M aqueous solution of hydrofluoric acid, HF, at 25.0 °C is 2.03. What is the value of Ka for HF?
4 answers
asked by
Anonymous
2,247 views
A 10.0-mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the
3 answers
asked by
Sandhya
2,080 views
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the
3 answers
asked by
Margaret
1,961 views
A 100.0 mL of 0.200 M methylamine, CH3NH2, is titrated with 0.100 M HCl. Calculate the pH after 70.0 mL of 0.100 M HCl has been
3 answers
asked by
Donna
1,854 views
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.140 M HClO(aq) with 0.140 M KOH(aq).HClO is a
3 answers
asked by
Emma
1,812 views
What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make
3 answers
asked by
emoni
1,733 views
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The
3 answers
asked by
Francesca
1,597 views
SALT HYDROLYSIS
1.) Calculate the pH of a 0.24M sodium formate (HCOONa) solution. Kb=5.9x10^-11. 2.) Calculate the pH of 0.25M
3 answers
asked by
jaycab
1,534 views
Calculate the pH for each of the following points in the titration of 50.0 mL of a 1.8 M H3PO3(aq) with 1.8 M KOH(aq).
before KOH
4 answers
asked by
Sofia
1,524 views
If the Ka of a monoprotic weak acid is 4.5x10^-6 what is the pH of a .10M solution of this acid.
I don't even know how to start
7 answers
asked by
Molly B
1,527 views
A certain indicator, HA, has a Ka value of 6.3 × 10-8. The protonated form of the indicator is blue and the ionized form is
3 answers
asked by
jjhjhhjhk
1,509 views
If you need to prepare 250.0 mL of a pH 5.00 buffer that has a total buffer concentration of acetic acid + sodium acetate of
4 answers
asked by
Natalie
1,508 views
How much of NaOH (in grams) is needed to prepare 546 mL of solution with a pH of 10.00 ?
3 answers
asked by
Sara
1,490 views
Pages
1
2
3
4
5
6
7
8
9
10
Parent Categories (27)
Analytical Chemistry
Aqueous Solutions
Biochemistry
Chemical Compounds
Chemical Equilibrium
Chemical Reaction
Chemical Reactions
Chemical Solutions
Chemistry
Chemistry Education
Equilibrium
General Chemistry
Inorganic Chemistry
Molecules
Organic Chemistry
Physical Chemistry
Science/Education/Chemistry
Solution Chemistry
Solution Preparation
Solutions
Solutions and Buffers
Solutions and Concentrations
Solutions and Mixtures
Solutions and Mixtures, Sub-sub-category: Acid-Base Chemistry
Solutions and Stoichiometry
Spectrophotometry
Stoichiometry