Number of results: 10,352
chemistry
What is the percent ionization of 0.025 M chlorous acid, HClO2 solution? Ka HClO2 = 1.1*10^(-2) Answer: 48% What I did: HClO2(aq) + H2O(l) -><- ClO2(aq) + H3O(aq) initial-change-end table results: x^(2)/(.025-x)=1.1*10^(-2) x=1.6*10^(-2) % ionization = (1.1*10^(-...
Saturday, July 30, 2011 at 7:13pm by % ionization
12th grade
The series of H, Cl, and O acids are as follows: HClO4 = perchloric acid HClO3 = chloric acid HClO2 = chlorous acid HClO = hypochlorous acid The general rule is that the acid is stronger if it has more O atoms in a series such as this. HClO4, perchloric acid, is a very strong ...
Tuesday, July 27, 2010 at 10:29pm by DrBob222
Chemistry
A buffer was prepared by dissolving 22.61g of NaCLO2 into 0.100L of 4.00M aqueous HCLO2. Calculate the pH of the original Chlorous acid/chlorite ion buffer. Ka= 1.1 x 10^-2.
Monday, December 3, 2012 at 10:14am by May
Chemistry--To Rose
HClO is hypochlorous acid, The question was for chlorous acid, HClO2.
Wednesday, November 9, 2011 at 8:25pm by DrBob222
chemistry
How do you name this acid? HClO2 I found the answer but now I need to know N2F4. chlorous acid dinitrogen tetrafluoride
Saturday, December 16, 2006 at 4:08pm by Carter
AP CHEMISTRY
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. a)hydrobromic acid (HBr) b)chlorous acid (HClO2) c)benzoic acid (C6H5COOH)
Wednesday, February 29, 2012 at 10:35pm by DANNY
chem
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH. chlorous acid (HClO2) benzoic acid (C6H5COOH)
Saturday, March 23, 2013 at 6:28pm by hannah
Chemistry
HClO2 is a weak acid. HClO2 + H2O ==> H3O^+ + ClO2^- Ka = (H3O^+)(ClO2^-)/(HClO2) Set up an ICE chart, calculate (H^+) and convert that to pH.
Monday, March 8, 2010 at 8:22pm by DrBob222
chemistry
a) carbon monoxide. b) no such animal. You may mean HClO2 which is chlorous acid.
Tuesday, February 8, 2011 at 2:55pm by DrBob222
Chemistry
You might want to look up Kb or an amide vs Kb for NH3. NH3 is the stronger base. Compare Kb for each. HClO3 and HClO2 are acids. HClO3 is the stronger acid; therefore, HClO2 is the stronger base. Compare Ka values. HClO2 has a Ka, HClO3 is a strong acid. Cl3CCOOH is a ...
Tuesday, November 20, 2007 at 1:51am by DrBob222
chemistry
You need to know the name of acids. Salts are named for the acid from which the salt is derived. We'll do that first. HCl hydrogen chloride HClO hypochlorous acid HClO2 chlorous acid HClO3 chloric acid HClO4 perchloric acid. For the salts of those acids, the binary is -ide...
Thursday, November 20, 2008 at 11:59am by DrBob222
chemistry
Which weak acid would be best to use when preparing a buffer solution with a pH of 8.50? 1) an acid with Ka=3.3x10^-9 2) an acid with Ka=5.0x10^-4 3) an acid with KA=6.3x10^-6 4) an acid with Ka=5.0x10^-7 5) an acid with Ka=4.0x10^-5 6) an acid with Ka=2.0x10^-10
Monday, April 8, 2013 at 3:31pm by Anonymous
Chemistry-Urgent Help Please
I don't know any tricks for remembering them unless it is to use them often enough that they become second nature. -ide names binary compounds (two atoms to the molecule such as NaCl-sodium chloride or CaC2-calcium carbide). The easiest way to describe the salts is to know...
Thursday, March 5, 2009 at 9:33pm by DrBob222
Chemistry
Of HClO3 and HClO2, HClO2 is the weaker acid; therefore, ClO2^- is the stronger base.
Tuesday, November 20, 2007 at 1:51am by DrBob222
CHEMISTRY
........HClO2 + H2O ==> H3O^+ + ClO2^- I.....0.120..............0.......0 C........-x..............x.......x E.....0.120-x............x.......x Substitute the E line into the Ka expression for HClO2 and solve for x = (H^+), then convert to pH = -log(H^+)
Saturday, February 9, 2013 at 11:00pm by DrBob222
chemistry
Buffers are composed of a weak acid and its salt OR a weak base and its salt. ii will do it. NaOH reacts with HClO2 to form NaClO2 and there is some HClO2 un-reacted. That makes a weak acid and its salt. iii is a salt and the weak acid.
Sunday, March 7, 2010 at 1:10am by DrBob222
Chemistry
You're right. HCl is the strongest acid. Note that all of the other acids are weak and have a Ka. Look in your text for Ka for each. Then rank the Ka values from weak to strong. The smallest Ka will be the weakest acid. #2. All of these are salts and K^+ is not hydrolyzed...
Sunday, October 23, 2011 at 12:07pm by DrBob222
chem
NaOH + HClO2 ==> NaClO2 + H2O so the pH at the equivalence point is determined by the hydrolysis of NaClO2 (actually the hydrolysis of the ClO2^-. The (ClO2^-) = 0.0444M. If you don't know how to do this I can show you. .........ClO2^- + HOH ==>HClO2 + OH^- I...
Saturday, March 23, 2013 at 6:28pm by DrBob222
last proofreading for the weekend
Here is a good lesson in suffixes and prefixes. "normal" acid is stem + ic. 1 less O, change ic to ous. 2 fewer O, add prefix of hypo...+ ous 1 more O, add prefix per to normal. For example. HClO4 PERchlorIC acid (Per + stem + ic) HClO3 chlorIC acid (stem + ic)(...
Saturday, March 8, 2008 at 10:29pm by DrBob222
chemistry
An unknown weak acid with a concentration of 0.32 M was found to have a pH of 2.7. Using the table of dissociation constants (Ka) below, determine what the likely identity of the acid is. Explain how you got your answer (hint - calculate the Ka in the same way you did for ...
Monday, March 25, 2013 at 12:48am by Anonymous
chemistry
Given the table of Ka values on the right below, arrange the conjugate bases in order from strongest to weakest. Acid Ka HClO 3.5 e-8 HClO2 1.2 e-2 HCN 6.2 e-10 H2PO4- 6.2 e-8 A. ClO2-, ClO¬-, HPO42-, CN- B. ClO2-, HPO42-, ClO¬-, CN- C. CN-, HPO42-, ClO-, ClO2¬- D...
Monday, November 29, 2010 at 12:01am by linda
Chemistry
You have the Ka for the weak acid is Ka = (H^+)(A^-)/(HA) If we solve this for (H^+) we get ((H^+) = Ka*(HA)/(A^-) At the exact half-way mark to the equivalence point, the acid that is left (not yet neutralized) exactly equals the salt formed; therefore, (HA) = (A^-). Thus, (H...
Friday, March 12, 2010 at 7:28pm by DrBob222
chemistry
Let's call acetate, Ac^- just to save some typing. Ac^- + HOH ==> HAc (acetic acid) + OH^- Kb for acetate = (Kw/Ka) where Ka is the acid constant for acetic acid. Kb = (Kw/Ka) = (HAc)(OH^-)/(Ac^-) Let HAc = x = OH, then (Kw/Ka) = x^2/Ac^-. Kw you know. Ka you know. ...
Monday, November 15, 2010 at 12:20am by DrBob222
Chemistry
In a 1.760 M aqueous solution of a monoprotic acid, 3.21% of the acid is ionized. What is the value of it's Ka? x=1.760M * 3.21/100 - .0565M Ka expression is Ka= {[H+][A-]} / [HA]
Sunday, March 18, 2012 at 10:58pm by Jamie
Chemistry
which of the following statements are true? a) For an acid H-O-A : the greater the electronegativity of A, the weaker the acid HA b) For an acid H-A : the weaker the H-A bond, the stronger the acid H-A c) HF is a stronger acid than HCl d) HClO4 is a weaker acid than HClO2 e) ...
Thursday, October 15, 2009 at 2:20pm by Anonymous
CHEMISTRY LAB urgent assistance
Start with the acid dissociation equation: HAc -> H+ + Ac- Ka is then [H+][Ac-]/[HAc] {given in the question} at the start HAc -> H+ + Ac- and we start from A mole/L and B mol/L for the acid and buffer A M ___0__ B M at the end HAc -> H+ + Ac- A-x____x___B...
Thursday, September 22, 2011 at 7:33am by Dr Russ
Chemistry
Classify the following 3 acids in order of increasing acidity: Acid 1:Ka = 8 x 10-6
 Acid 2:Ka = 6 x 10-4
 Acid 3:Ka = 9 x 10-11
Sunday, May 13, 2012 at 9:32pm by Andrea
Chemistry -- Please Help!!
Find the pH of a mixture of .150 M HF(aq) solution and 0.100 M HClO2(aq) HF + H2O <--> F- + H3O+ Ka= 3.5*10^-4 So I will show my attempt below... [HF] [F-] [H3O+] I .150 0 0 C -x +x +x E .15-x x x Ka= [F-][H3O+]/[HF] 3.5*10^-4= x^2/(.150-x) assume x is small so...
Monday, April 26, 2010 at 7:06pm by Erin
Chemistry -- Please Help!!
Technically, there is no way to get a firm solution to the problem because the problem doesn't specify the mixture's composition. Your calculation is correct, as far as it goes, and your observation is correct also. According to my tables, HClO2 is a stronger acid than...
Monday, April 26, 2010 at 7:06pm by DrBob222
Chemistry
We will call weak acid A as HA. pH = 2.20; therefore, H^+ = 6.31E-3 ...........HA ==-> H^+ + A^- I........0.0870.....0.....0 C...........-x.......x.....x E......0.0870-x.....x......x You know x = 6.31E-3; therefore, Ka = (H^+)(A^-)/(HA) Ka = (6.31E-3)(6.31E-3)/(0.08069...
Friday, April 12, 2013 at 12:46pm by DBob222
Chemistry Acid Question Ka
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. Calculate the Ka for the acid.
Sunday, April 22, 2012 at 10:52pm by RZeal
Plz -- Chem Help
Question.. Nicotinic acid (niacin) is a monoprotic acid with the formula HC6H4NO2. A solution that is 0.012M in the nicotinic acid has a pH of 3.39 at 25C. what is the acid-ionization constant, Ka and pKa for this acid at 25C? Attempt.. HC6H4NO2 <----> C6H4NO2...
Sunday, March 15, 2009 at 3:35pm by Rushi
Urgent Chem Help
Question.. Nicotinic acid (niacin) is a monoprotic acid with the formula HC6H4NO2. A solution that is 0.012M in the nicotinic acid has a pH of 3.39 at 25C. what is the acid-ionization constant, Ka and pKa for this acid at 25C? Attempt.. HC6H4NO2 <----> C6H4NO2...
Sunday, March 15, 2009 at 3:34pm by Saira
Chemistry
Need help with AP chemistry, specifically Acids and Bases The acid ionization constant, Ka, for propanoic acid, C2H5COOH, is 1.3  10 -5 . (a) Write the expression for the acid-dissociation constant, Ka for propanoic acid. (b) Calculate the hydrogen ion ...
Monday, April 9, 2012 at 8:59pm by Sam
Chemistry
I can't check your answers because you didn't provide the Ka for HClO2. I don't have it listed in any of my references.
Sunday, April 3, 2011 at 11:11pm by DrBob222
Chemistry
I mean how it effects the acid-dissociation constant(Ka). How does water effect the Ka value of a weak acid?
Monday, October 27, 2008 at 11:45am by Jessica
chemistry
The acid is acetic acid. Either in your problem or in your text the Ka should be listed as close to 1.8E-5 which is a pKa of 4.74 (pKa = -log Ka). Use the value in your text or notes, not the one I used. The base is acetate. The acid is acetic acid in the HH equation.
Sunday, December 5, 2010 at 8:58pm by DrBob222
Chemistry
Known: Cyanaocetic acid Ka=3.55*10^-3 ionization equation: HC3H2NO2<==> H^+ + C3H2NO2^- Unknown: pH of 0.4M of Cyanaocetic acid I can't figure out how to calculate this. I only knew how to calculate the pH value of an acid with a known Ka, but not in this ...
Monday, April 20, 2009 at 11:42pm by anonymous
Chemistry
pKa is the pKa for acetic acid. Since Ka for acetic acid is about 1.8 x 10^-5, the pKa is -log Ka = about 4.75 or so. You need to look up Ka for acetic acid in your text or notes and take the negative log of that value.
Sunday, July 19, 2009 at 7:24am by DrBob222
Chemistry
You must recognize that this is a mixture of two weak acids; i.e., formic acid and acetic acid. I looked up Ka for both and used 1.77E-4 for Ka HCOOH and 1.8E-5 for Ka CH3COOH. Calculate the H^+ from the strong acid, then add the H^+ from the weak acid. Formic acid first since...
Sunday, February 26, 2012 at 2:27am by DrBob222
Chem
SrSO4, CuCN, and Ni(OH)2 are more soluble in acidic solution than in pure water. If you don't understand what basic anions are, then look at it this way. Which anions will hydrolyze with H2O to form a WEAK acid when added to H^+; i.e., an acid that has a Ka (not a strong ...
Thursday, May 2, 2013 at 7:28pm by DrBob222
chemistry
Based on what I can find on the internet, ascorbic acid is a monoprotic acid. If that is so, then let's call ascorbic acid HC. Then HC ==> H^+ + C^- Ka = ((H^+)(C^-)/(HC) If pH = 2.40, then (H^+) = 0.00398/ (C^-) is the same. (HC) = 0.2 = 0.00398 Plug in the Ka ...
Sunday, April 6, 2008 at 12:46am by DrBob222
Chemistry
I don't know what value you used for Ka for HClO2. I looked on the net and found 0.012 in two places. It would have been better if you showed your work, then I could find the trouble. I suspect you didn't solve the queadratic but I could be mistaken. The equation ...
Monday, March 8, 2010 at 8:22pm by DrBob222
chemistry
Weak acid is HA. HA ==> H^+ + A^- Ka = (H^+)(A^-)/(HA) Convert pH to H^+, substitute into Ka expression for Ka and solve for Ka.
Friday, September 24, 2010 at 4:43pm by DrBob222
chemistry
Hey - just look up the Ka (or Kb respectively) values for each compound, and see which is bigger. Stronger acid = bigger Ka and that will dictate which direction it will go in. In this case, H3PO4 is the strongest acid (highest Ka) and therefore the direction of that reaction ...
Sunday, March 8, 2009 at 1:58am by Julia
chemistry
A 0.25 mol/L solution of benzoic acid, KC7H5O2 and antiseptic also used as a food preservative, has a pH of 2.40. Calculate the Ka of benzoic acid at SATP My work: C6H5COOH --> C6H5COO^- + H^+ Ka = (C6H5COO-)(H+)/ C6H5COOH I know my next steps are to use pH = log(H+) to...
Monday, April 7, 2008 at 5:15pm by Dustin
Chemistry Very Urgent!!
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 = -log(H^+) You know pH. Convert that to (H^+). (H^+)=(A^-) so plug those into the expression for Ka. (HA) = 0.035 M - (H^+). Plug that in. ...
Monday, April 2, 2007 at 11:35pm by Paul
Chemistry
Let's just call this acid HA. It's the salt that is hydrolyzing, so A^- + HOH ==> HA + OH^- Kb = Kw/Ka = (HA)(OH^-)/(A^-) You know Kw, Ka is what you want, (HA)=(OH^-) and you can get the OH from the pH. After you find Ka, use that as you would a weak acid ...
Thursday, January 21, 2010 at 4:24pm by DrBob222
Chemistry
An acid HA has Ka = 2.28 x 10^-4. The % ionisation of this acid in a 0.170 M solution of the acid in water is? An acid HA has Ka = 2.28 x 10^-4. The % ionisation of this acid in a 0.170 M solution of the acid in water is closest to a. 2.930 % b. 3.662 % c. 2.564 % d. 0.498 % e...
Thursday, May 26, 2011 at 9:21pm by Cheryl
chemistry
Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
Thursday, January 20, 2011 at 5:19am by jaycab
chemistry
Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
Thursday, January 20, 2011 at 5:19am by jaycab
chemistry
Methanoic acid HCO2H(aq) also known as formic acid, is partly responsible for the characterisitic itchy rash produced by the leaves of the stinging nettle plant. Calculate the pH of 0.150 mol/L methanoic acid. The Ka for methanoic acid is 1.8 x 10^-4. My Work: Lets call ...
Sunday, April 6, 2008 at 10:47pm by Sarah
chemistry
A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of ...
Thursday, January 20, 2011 at 3:37am by jaycab
chemistry
Lactic acid, HC3H5O3(aq) is a weak acid that gives yougurt its sour taste(Yeeeeecccckkk). Calculate the pH of a 0.0010 mol/L solution of Lactic acid. The Ka for lactic acid is 1.4 x 10^-4 For Further Reading chemistry - DrBob222, Saturday, April 5, 2008 at 7:39pm Let's ...
Sunday, April 6, 2008 at 10:42pm by Sarah
Chem
Acetic acid is 3% dissociated in a 0.02M solution. Give the concentrations of each of the two ions, the acetic acid, and the Ka for acetic acid. HC2H3O2 ==> H^+ + C2H3O2^- So (H^+) = 0.02*0.003 = ?? (C2H3O2^-) = 0.02*0.003 = ?? Plug into Ka expression and solve for Ka. ...
Saturday, July 14, 2007 at 2:20pm by Lizette
Chemistry
Given acidity constant,Ka of benzoic acid is 6.28 X 10^-5. pH of 0.15 molar solution of this acid is ? Here is my method: Benzoic acid is a weak acid,hence it dissociates very little. So: C6H5COOH---> C6H5COO- + H+ [H+] and [C6H5COO-] are yet to be calculated,so let ...
Friday, March 23, 2012 at 12:28am by Meenaakshi
Chem
What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH<--> C6H5COOH Once I...
Wednesday, February 27, 2008 at 4:22pm by Sarah
chemistry
Two comments. #1. You don't means nitric acid. You mean nitrous acid, HNO2. #2. You found the Ka for HOCl, HNO2, and C6H5COOH. You want Kb (not Ka) for the anion; i.e., OCl^-, NO2^-, and C6H5COO^-. Easy to do. KaKb = Kw. You know Kw, you find Ka in the tables for the ...
Tuesday, April 8, 2008 at 8:15pm by DrBob222
chem
You COULD work each one for pH and see which is the lowest but that isn't necessary. I'll show you how to do one of them, HF since it is first. .............HF ==> H^+ + F^- initial......1.0.....0.....0 change.......-x......x......x equil......1.0-x.....x..........
Friday, January 20, 2012 at 4:00pm by DrBob222
chemistry
Look in your text or notes at the Ka for weak acids. If a Ka is listed it is a weak acid. If not it is a strong acid (or an incomplete table.
Wednesday, April 28, 2010 at 2:52pm by DrBob222
Chem 2
What is the approximate value of the K for the neutralization of nitrous acid with ammonia? Ka for the acid is 0.00045 and Kb for the base is 0.000018. Do I multiply Ka*Kb?
Thursday, February 28, 2008 at 10:30pm by Sarah
Chemistry
The Ka for a particular weak acid is 4.0 x 10-9. Calculate the pH of a 0.040 M solution of this acid. whats the relation b/w Ka and pH?
Saturday, November 1, 2008 at 2:51am by A.A
Chemistry
An 0.0284 aqueous solution of lactic acid is found to be 6.7% ionized. Determine Ka for lactic acid. HC3H5O3 + H2O <-- --> H3O^+ + C3H5O3^- Ka =? Thanks.
Monday, August 10, 2009 at 12:46am by Sev
Chemistry
(a) Explain what is meant by a weak acid. Methanoic acid (HCO2H) has a numerical value of Ka(T) at 298K of 1.60 × 10-4 (b) Write an expression for Ka(T) of methanoic acid, and state its units. (c) What is the pH value of a 0.10 mol dm-3 aqueous solution of methanoic acid...
Sunday, April 22, 2012 at 3:44pm by Henry
College Chemistry
"What is the pH of a solution that is 0.50 M in sodium acetate and 0.75 M in acetic acid? (Ka for acetic acid is 1.85 x 10-5)." Would i use the Ka expression formula??
Tuesday, October 19, 2010 at 11:02pm by James
College Chem II
Benzoic acid = HBz HBz ==> H^+ + Bz^- Ka = (H^+)(Bz^-)/(HBz) Set up an ICE chart, substitute into the Ka expression, and solve for (H^+), then convert to pH. You will need to look up the Ka for benzoic acid.
Sunday, March 7, 2010 at 6:07pm by DrBob222
chemistry
Reading the pH at the 1/2 way point to the equivalence oint will give you the Ka if you set pH = -log(H^+) Reading the pH will give you the pKa of the acid directly. Try this. For an acid HA that ionizes HA ==> H^+ + A^- Ka = (H^+)(A^-)/(HA) at the half way point, (A...
Tuesday, April 8, 2008 at 11:39pm by DrBob222
Chem 2
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 ionization is HB ==> H^+ + B^- To start (HB) = 0.15 (H^+) = 0 and (B^-) = 0 After ionization, (H^+) = x but that is found by converting pH to (...
Thursday, July 19, 2007 at 1:47am by Jess
Chemistry
ide, ite, and ate are endings for SALTS; i.e., a metal + non-metal. ide is for binary compounds. Binary compounds are those compounds composed of two elements. NaCl, LiBr, Na2O, Mg3N2 are -ide compounds; sodium chloride, lithium bromide, sodium oxide, magnesium nitride, etc. ...
Thursday, March 3, 2011 at 5:55am by DrBob222
Chemistry
The pH at the halfway point of a weak acid/srong base or weak base/strong acid is pH = pKa. Look at the Ka expression for a weak acid. Ka = (H^+)(A^-)/(HA). Now solve this for H^+. (H^+) = Ka*[(HA)/(A^-)]. When you are halfway there, the (HA) = (A^-); therefore, Ka = (H^+). If...
Saturday, December 1, 2012 at 3:03pm by DrBob222
chemistry
Two problems with what you did. 1. %ion = [(H3O^+)/0.025]*100 = ?? 2. Your equation is set up correctly; i.e., x^2/(0.025-x) = Ka. However, with Ka so large and (HClO2) so small, you MUST solve the quadratic equation. That is, you may not assume 0.025-x = 0.025. 3. I get 47.9...
Saturday, July 30, 2011 at 7:13pm by DrBob222
chem
Let's call sorbic acid HSorb. HSorb ==> H^+ _ Sorb^- Ka = (H^+)(Sorb^-)/(HSorb) = Ka. So (H^+) = x (Sorb^-) = x (HSorb) = 0.37 - x Substitute into the Ka expression and solve for x. Note: It would be a good idea to convert pKa to Ka first.
Sunday, February 21, 2010 at 5:22pm by DrBob222
Chemistry
Is the structure for chlorous acid H O Cl O or H Cl O ? O I was thinking that both could be correct but I am not 100% sure.
Wednesday, November 9, 2011 at 8:25pm by Hannah
Chemistry
Is the structure for chlorous acid H O Cl O or H Cl O ? O I was thinking that both could be correct but I am not 100% sure.
Wednesday, November 9, 2011 at 6:21pm by Hannah
12th grade
Which acid is stronger: HClO2 or HClO3? Can you also explain why?
Tuesday, July 27, 2010 at 10:29pm by Kat
chem 12
You start over. Benzoic acid is an acid, not a base. Let's call benzoic acid HB. ..........HB ==> H^+ + B^- init.....0.15.....0.....0 change....-x......x.....x equil....0.15-x...x.....x Ka + (H^+)(B^-)/(HB) Substitute the equilibrium line above into the Ka ...
Tuesday, October 11, 2011 at 2:03pm by DrBob222
chemistry
Yes to the first question. (H^+) = 10^-pH. At the half way point, which is what you had, then Ka = (H^+ or pKa = pH but that is only true at the half way point. You can see for a weak acid, such as HA HA ==> H^+ + A^- and Ka(H^+)(A^-)/(HA). Solving for (H^+) we get (H...
Thursday, April 17, 2008 at 3:04pm by DrBob222
ap chemistry
I and IV are strong acids. HF is the most common weak acid, and this has to do with electronegativity of F. LiOH is a strong base, I think. And HCLO2 is a weak acid; O's have to outnumber the H's by two or more.
Thursday, February 28, 2013 at 10:00pm by Devron
chemistry
Calculate [acetate] of 0.057 mol/L solution of acetic acid of Ka = 1.76x10^-5 i know to find Ka it's: Ka= products/reactants so i tried doing an ICE table with the equation to be: CH3CO2 + H2O <--> CH3COOH + H am i on the right track? if not...help please!
Wednesday, July 28, 2010 at 12:06am by Kat
CHEM HELP!
Nicotinic acid (niacin) is a monoprotic acid with the formula HC6H4NO2. A solution that is 0.012M in nicotinic acid has a pH of 3.39 at 25*C. What is the acid-ionization constant, Ka and pKa for this acid at 25*C?
Tuesday, March 17, 2009 at 6:36pm by Ashley
College Chemistry
nicotinic acid (niacin) is a monoprotic acid with the formula HC6H4NO2. A solution that is 0.012M in the nicotinic acid has a pH of 3.30 at 25C. what is the acid-ionization constant, Ka and pKa for this acid at 25C?
Thursday, March 5, 2009 at 2:35pm by Anonymous
chem
Ice table ? I haven't heard of that term in awhile. Well since acetic acid is a weak acid and NaOH is a strong base... 120ml 0.15M acetic acid 30ml 0.2M NaOH -You need Ka for the weak acid. (for acetic acid Ka= 1.8x10^-5) steps: 1. Determine if moles H+ or moles OH- is in ...
Monday, August 27, 2007 at 10:42pm by ~christina~
Chemistry
Yes and no. (acid) is not 1.8E-5; that's ka for acetic acid. You put 250*0.56 for base and mL*0.500 for acid; solve for mL acid.
Tuesday, April 10, 2012 at 10:43am by DrBob222
chemistry
The Ka of a monoprotic weak acid is 7.25 × 10-3. What is the percent ionization of a 0.167 M solution of this acid? If the concentration is more than 1000 times greater than the Ka, then you can make an assumption that simplifies the algebra needed to solve the problem. ...
Wednesday, April 10, 2013 at 11:57am by sara
chemistry
Write the benzoic acid ionization. Write the Ka expression. Use pH = =log(H^+) to calculate (H^+). Substitute into Ka expression and determine Ka.
Saturday, April 5, 2008 at 6:42pm by DrBob222
Chemistry
A 0.23 M solution of a weak acid has a pH of 2.89. What is the Ka(acid ionization constant)for this acid?
Tuesday, November 16, 2010 at 8:52pm by Sarah
Chemistry
A 0.23 M solution of a weak acid has a pH of 2.89. What is the Ka(acid ionization constant)for this acid?
Tuesday, November 16, 2010 at 5:03pm by Sarah
apchem PLease Answer
HOCl + H2O ==> H3O^+ + OCl^- Kiki--I just don't understand what your problem is with HOCl and HOBr. These are weak acids just like acetic acid, oxalic acid, phosphoric acid, etc. They ionize partially and the have Ka. Their salts ionize in water just as acetate ion ...
Monday, April 19, 2010 at 6:26am by DrBob222
Chemistry! Please Help!
Let's call propionic acid HP, then it will ionize as HP ==> H^+ + P^- First convert pH = 2.50 to (H^+) by pH = -log(H^+). Then set up the expression for Ka. Ka = (H^+)(P^-)/(HP). You know (H^+) now from the pH calculation. You know (P^-) because it equals the same ...
Thursday, February 12, 2009 at 7:46pm by DrBob222
Chemistry
Part A: Unknown Acid use 1gram and mix with 120 mL of distilled water Determine the concentration of the acid by titrating with 0.0998 M of NaOH Concentration of NaOH= 0.0998M Volume of NaOH= 3.5 mL # moles of NaOH= Initial Concentration of Weak Acid- Show Calculation of Ka ...
Wednesday, March 24, 2010 at 3:40pm by Saira
chemistry
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 acetic acid is 1.76 × 10-5.
Wednesday, November 24, 2010 at 12:44pm by jack
chemistry
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 acetic acid is 1.76 × 10-5.
Wednesday, November 24, 2010 at 10:22am by jack
chemistry
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 acetic acid is 1.76 × 10-5.
Tuesday, November 23, 2010 at 11:22pm by jack
Chemistry
Sodium iodate is the salt of a strong base (NaOH) and a weak acid (HIO3). So this salt hydrolyzes as in the last problem I posted. The only difference is that this is a STRONG weak acid with Ka a relatively large value of about 0.18 or so. You need to confirm that. That means ...
Monday, April 14, 2008 at 11:00pm by DrBob222
Chemistry(Please help)
You want to find Kb for acetate. That is Kw/Ka and Ka is for acetic acid.
Saturday, April 7, 2012 at 10:54pm by DrBob222
Chemistry(Please just check, thank you)
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 stronger acid than HF, which is stronger than HOCL, then the order of strengths of the conjugate bases of these acids is? My answer is CLO2^-^ &...
Saturday, March 24, 2012 at 1:50pm by Hannah
Chemistry 12
Thanks so much :) So if we were to find the Ka, then we would use the ka on the acid side of the chart?
Friday, January 25, 2013 at 12:40am by Shreya
Chemistry
What is the [H+] of a 0.1 M malonic acid with a Ka of 10^-9 solution? I thought it was just (Ka x Ca)^(0.5), but that doesn't get me a pH of 5.
Saturday, May 7, 2011 at 9:34pm by Ed
Chemistry- Buffers
-log Ka = pKa which may or may not be = pH. Ka is a measure of how strong/weak the acid is.
Sunday, December 5, 2010 at 9:53pm by DrBob222
Chemistry
For the salt of a weak acid and a weak base, (H^+) = sqrt(KwKa/Kb). For NH4OCl, that is about 4 x 10^-9 or pK about 8.4 (which is slightly basic). What it boils down to, if you look at the equation, is the Kw part will give neutral. If Ka = Kb, the solution is neutral. If Ka&...
Tuesday, May 18, 2010 at 8:14pm by DrBob222
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