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April 20, 2014

Search: Chemistry/pH- Weak Acid

Number of results: 106,066

chemistry
Your answer may or may not be right. However, the reasoning is incorrect. You know that if a 0.20 M acid is a strong acid that it must ionize completely; therefore, the (H^+) will be 0.2M and the pH will be about 0.7. The pH isn't 0.7 so it must b a weak acid. Does that make ...
Wednesday, March 3, 2010 at 3:51am 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
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
The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in Appendix E of your textbook...
Friday, April 12, 2013 at 12:46pm by Maddie

chemistry
Correct on 1. Correct on 2. Correct on 3. To be a buffer, the solution must be a weak acid and its salt (conjugate base) OR a weak base and its salt (conjugate acid). Thus, adding a strong base, such as NaOH, to a weak acid, such as acetic acid, forms sodium acetate and you ...
Monday, November 8, 2010 at 1:48am by DrBob222

Chemistry
To prepare an effective buffer in a PH range less than 7 ,it is advisable to select a weak acid-conjugate base pair in which the pK(a) of the weak acid equals the desired PH (+-)1 Over what PH range is the acetic acid-acetate ion buffer most effective ?K(HC2H3O2)=1.8x10^-5 ...
Sunday, October 23, 2011 at 1:44pm by Queenking

chemistry
When a strong acid is added (exactly neutralized) to a strong base, the salt produced is neutral (neither cation nor anion is hydrolyzed) and the pH = 8. When a weak acid and a salt of the weak acid are present in solution, you hve a buffered solution and you must use the ...
Sunday, July 11, 2010 at 11:12pm by DrBob222

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-Dr Bob help!!
0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of 0.250 M HX
Wednesday, April 4, 2012 at 2:02pm by clayton

chemistry
What does pH stomach and pH instestines mean? Is that the average pH in stomach and intestines for humans? If so, what does it have to do with the problem. If the pKa of the drug is pKa = 2.1, it is a weak acid with K = 7.9E-3, relatively strong as weak acids go but weak none ...
Monday, March 19, 2012 at 11:13pm by DrBob222

Chemistry
Let me correct you Nan. You may just need to know which answer to choose; however, we try to give you the how without giving the answer. I gave you the HOW to work the problem, I did not give you the answer. For Aaron, pH = 4 is NOT necessarily a weak acid. A pH = 4 means the ...
Saturday, October 22, 2011 at 7:26pm by DrBob222

Chemistry
Acetic acid is a weak acid; sodium acetate is a salt of a weak acid. The combination makes a buffered solution. You calculate pH from the Henderson-Hasselbalch equation.
Sunday, June 12, 2011 at 11:01pm by DrBob222

chemistry
2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate the pH of the solution formed by adding 10...
Sunday, March 25, 2012 at 6:06pm by bob

Chemistry/pH- Weak Acid
in response to Chemistry/pH- Weak Acid. but the rule of 5%? 0,0100/(1.00x10^-4) =100% The aproximation you do is not valid...or? Ka= (1,0*10^(-4))^2/(x-1*10^(-4) )=1,00*10^(-6)....I got c=0,0101M :-(
Monday, August 18, 2008 at 9:24am by Mary

Chemistry
PLEASE HELP!! 40 mL of 0.1 M solution of a weak acid (adjusted to a pH of 7.75) is titrated with 0.2 M HCl to a final pH of 2.1. Once the pH of the weak acid reaches 2.1, it is then titrated with 20 mL of 0.25 NaOH. What is the final pH of the solution? pKa values are 2, 6, ...
Thursday, October 17, 2013 at 7:17pm by AA

Chemistry
In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base d.the hydrolysis of the conjugate base of the weak ...
Thursday, May 26, 2011 at 8:56pm by Cheryl

chemistry
a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used the formula pH=kpa+log(base/acid) Ph=3.89+log(6....
Thursday, November 25, 2010 at 1:52pm by help

chemistry
a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used the formula pH=kpa+log(base/acid) Ph=3.89+log(6....
Thursday, November 25, 2010 at 1:55pm by help

chemistry
if 0.4M NaOH is titrated with 0.4M HF, how do we calcualte the ph at equivalence. The book assumes each is 1L, but why do we use 1L * chemistry - Dr.Jim, Thursday, November 11, 2010 at 5:31am HF is a weak acid, so you need the dissociation constant. The pH at the equivalence ...
Thursday, November 11, 2010 at 4:03pm by flame

Chemistry
A buffer is prepared by mixing 110. mL of 0.442 M HCl and 0.545 L of 0.400 M sodium acetate. How many grams of KOH must be added to 0.500 L of the buffer to change the pH by 0.10 units? The pH I have calculated to be 5.28. What do I to figure this out? I have a problem with ...
Monday, April 2, 2007 at 12:58pm by Christina

CHemistry
I didn't work it out. I think it is true, too, but not for the reasons you gave. The acid by itself has a certain pH. The mixture consists of a weak acid (acetic acid) and its salt(the sodium acetate which by the way is a base); therefore, this is a buffered solution. Most, if...
Monday, May 5, 2008 at 5:26pm by DrBob222

chemistry 12
The pH of a certain acid having a concentration of 0.20M was measured. The pH was 2.50. Was this a strong acid or weak acid?
Thursday, October 13, 2011 at 12:37pm by Mike

Chemistry pH
A 0.60 M solution of a weak acid, HA, has a pH of 3.72. What is the percentage ionization of the acid? What is the value of Ka for the acid?
Thursday, April 17, 2014 at 2:17pm by Penny

Chemistry
In its simplest form, a buffered solution resists a change in pH. An unbuffered solution does not. For example, a buffered solution of acetic acid and sodium acetate will change pH only slightly when 1 ml of strong acid (HCl for example) is added. But 1 mL HCl added to an ...
Sunday, March 23, 2008 at 9:16pm by DrBob222

Chemistry
1. As the strength of a weak acid increases, the proportion of ions to molescules increases or decreases? ... I think that it will increase. Is this right? 2. As the as the concentration of a weak acid increases, the pH... decreases? Is decreases correct? 3. at the same ...
Friday, May 4, 2012 at 9:11am by April

Chemistry
The pH of a 0.100 M solution of an aqueous weak acid (HA) is 4.00. What would the Ka for the weak acid be?
Monday, April 16, 2012 at 7:17pm by Grace

Chemistry
1. You are correct. The strength of a weak acid is proportional to its dissociation constant, which is directly proportional to the concentration of ions and inversely proportional to the concentration of the undissociated acid molecules. 2. Yes, this is correct. The pH ...
Friday, May 4, 2012 at 9:11am by Phil

Chemistry
what is the concentration of a weak acid with a pH of 3.25, if the Ka of the weak acid is 1.6 x 10^-7 ?
Thursday, December 1, 2011 at 12:45pm by Cody

Chemistry
strong base: Ca(OH)2 highest pH KOH weak base: NH3 weak acid: HBrO strong acid: HCl lowest pH
Monday, April 16, 2012 at 5:24pm by DrBob222

General Chemistry
How do I calculate the ratio of weak base to weak acid in a methyl amine buffer solution at pH=10.645 and pH=11.645 and pH=9.645?
Monday, February 27, 2012 at 8:05pm by Nhi Song

Chm 2
The question asks, Consider the following weak acids and their Ka values Acetic acid Ka = 1.8x10^-5 Phosphoric acid Ka = 7.5x10^-3 Hypochlorous acid Ka = 3.5x10^-8 What weak acid-conjugate base buffer system from the acids listed is the best chouce to prepare the following ...
Tuesday, October 15, 2013 at 12:29am by Kyle

chemistry
The pH of a certain acid having a concentration of 0.20 M was measured. The pH was 2.50. Was this a strong or a weak acid? I answered it is a strong acid because strong acids have a lower pH. I am just not too sure if there is anything missing in my answer. Any help would be ...
Wednesday, March 3, 2010 at 3:51am by Billy

chemisty
0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of 0.250 M HX
Wednesday, April 4, 2012 at 5:35am by Clayton

chemistry
A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. A solution is created using 0.10M of a salt NaB ('B' being the anion of the weak acid HB) and 50.0 ml of 2.0M acid HB (assume no change in volume). What would be the pH of the solution and what would you call ...
Sunday, July 31, 2011 at 8:20pm by Hoot

chemistry
Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone explain this combination
Sunday, November 7, 2010 at 1:35am by poet

chemistry
Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone explain this ...
Monday, November 8, 2010 at 1:48am by poet

chemistry
With some difficulty. What level chemistry are you studying. This may be more than you ever wanted to know about H2SO4 but here are the facts (the correct answer is not given). If you consider H2SO4 a monoprotic acid the pH = -log(0.003) = 2.5 If you consider H2SO4 a diprotic ...
Saturday, March 17, 2012 at 7:23pm by DrBob222

chemistry
Give you the equation for what? Sodium lactate is the salt of a weak acid and a strong base and lactic acid is a weak acid. This COULD be a buffer solution. But it could be a lot of other stuff, too. If it's a buffer, the equation may be pH = pKa + log (base/acid).
Monday, January 11, 2010 at 9:37pm by DrBob222

chemistry 12
If the acid were a strong acid, the pH would be pH = -log(H^+) = -log(0.2) = about 0.7 and it is 2.50; therefore, it must be a weak acid.
Thursday, October 13, 2011 at 12:37pm by DrBob222

Chemistry
1 g of acid was mixed with 120 ml of distilled water and the solution was filtered into a clean dry beaker. A 25 ml aliquot of this solution was titrated with 0.1120 M NaOH. The pH of the acid was recorded to be 4.42. Calculate the initial concentration of the weak acid and ...
Monday, March 25, 2013 at 6:12pm by Annie

Chemistry
Equal moles of nitric acid (HNO3) and formic acid (HCOOH) were each dissolved in equal volumes of water. State and explain which of the resulting solutions would have the higher pH. Your answer should include an explanation of the terms strong acid and weak acid and a ...
Thursday, May 16, 2013 at 4:58pm by Ez

Chemistry
You are right. D is the correct answer. You are also correct that a good buffer is a weak acid or weak base and its conjugate base/acid. However, HCl is not a weak acid; therefore, it along with sodium chloride is not a good buffer. D is a good buffer because it is a weak acid...
Wednesday, March 20, 2013 at 6:47pm by DrBob222

Chemistry
I took 25 mL of an unknown weak acid and added it to 10 mL of NaOH solution. I measured the pH and got 2.88 with concentration of NaOH @ .0098 and weak acid at 0.0102. What is pKa for the acid?
Saturday, May 5, 2012 at 9:54pm by tc

Chemistry
.050 mole of weak acid (HA) is dissolved in enough water to make 1.0 L of solution. The pH of this solution is 3.50. What is the value of Ka for this weak acid?
Friday, April 6, 2012 at 5:52pm by Hannah

CHemistry
For the salt of a weak base (NH3) and a weak acid (HC2H3O2), the (H^+) = sqrt(KwKa/Kb), then convert (H^+) to pH. Another way, if you want to use logs is pH = 1/2(pKw + pKa - pKb). The latter is shorter if you know the pK values. I think both pKa and pKb are 4.74. I believe ...
Wednesday, December 8, 2010 at 4:46pm by DrBob222

chemistry
A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following statements best explains your prediction? 1. ...
Monday, March 31, 2014 at 4:23pm by bekah

chemistry
Buffers are solutions contg a weak acid and its salt or a weak base and its salt OR something that can form a weak acid/base and salt. b. Has weak acid,HF, and salt KF. c. Has weak base, NH3, and salt, NH4Cl. e. Has NaNO2 which is the salt of a weak acid and it contains HNO3 ...
Thursday, April 12, 2012 at 8:48pm 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 5:03pm 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 8:52pm by Sarah

Chemistry
A 0.60 M solution of a weak acid, HA, has a pH of 3.72. What is the percentage ionization of the acid? What is the value of Ka for the acid?
Wednesday, April 16, 2014 at 9:58pm by Anonymous

chemistry
A buffer solution is composed of 0.370M HA, a weak monoproctic acid, and 0.370M NaA, the sodium salt of the acid. The solution has a pH of 3.50. What is the Ka of the weak acid, Ha?
Monday, April 30, 2012 at 1:09pm by Cayla

Chemistry
The lower the pH of a weak acid, the: a. higher the concentration of the weak acid. b. higher the dissolved H2(g) concentration. c. higher the Ka of the acid. d. none of the above
Wednesday, June 5, 2013 at 10:57am by Anonymous

152
The pH of HClO at the beginning of the titration is calculated from HClO as a single weak acid. Additions of NaOH form NaClO, which is a weak acid and its salt, therefore, the Henderson-Hasselbalch equation is used. At the equivalence point, the acid is completely neutralized ...
Wednesday, March 31, 2010 at 7:36pm by DrBob222

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
Hello, I'm wondering what the difference is in method when it comes to finding the pH of a weak acid versus finding the pH of a strong acid? Thanks!
Monday, April 26, 2010 at 7:23pm by Rob

chemistry
For 0.250 M of weak acid (NaHS) the Kb is given by 1.22 x10-13 , calculate the pH of the weak base.
Saturday, April 18, 2009 at 5:12pm by lil'mama

Chemistry-pH problem
If a weak acid has a dissociation constant of 6.4 x 10(-6), what is the pH of a solution of this acid in 0.10 molar concentration?
Monday, December 13, 2010 at 2:47pm by Maddy

chemistry
do we have buffering region and ph=pka in any of these conditions: strong base vs strong acid strong base vs weak acid weak base vs strong acid weak base vs weak acid
Sunday, May 23, 2010 at 6:19pm by eng

Chemistry/pH- Weak Acid
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 pH of 4.000. What volume of water must be added to make the pH = 5.000? My Calculations: To calculate the concentration of x, I take the pH value -&...
Sunday, August 17, 2008 at 6:07am by Mary

Chemistry
Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75) I got pH= 3.88 ...
Sunday, February 27, 2011 at 12:49pm by Jon

General Chemistry-Acids/Bases
The first problem is a buffer problem. HF is a weak acid and NaF is the salt of the weak acid. Use the Henderson-Hasselbalch equation. The second problem is a strong acid/strong base problem. There are no ionization constants involved and you can go from molarities to H^+ and ...
Wednesday, November 26, 2008 at 2:18pm by DrBob222

Chemistry -- to Dr.Bob
No, because sodium acetate is the salt of a strong base and a WEAK acid, (as opposed to HCl which is a strong acid) so you just follow the steps I did. write the equation. You have mols NaOH You have mols acetic acid. So how much sodium acetate (the salt) is produced? What is ...
Friday, May 2, 2008 at 9:41pm by DrBob222

chemistry
A. The data and experimental details are too scant/vague to make sense of the questions. Your #1. The relative concns can be estimated by the ratio of the volumes used. Your #2. You would need mL and M of vinegar and mL of ammonia. I don't think the pH of either is needed. ...
Saturday, March 6, 2010 at 7:47am by DrBob222

chemistry
HF is a weak acid, so you need the dissociation constant. The pH at the equivalence point is found by calculating the pH of a 0.4M NaF solution (a hydrolysis problem). If you erroneously assume that HF is a strong acid, then the answer is simple. The pH at the equivalence ...
Thursday, November 11, 2010 at 2:29am by Dr.Jim

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
hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M NaOH Base (in mL) is ...
Monday, July 12, 2010 at 2:31pm by THOMAS

Chemistry
I have an assignment Q A 0.1 mol L-1 water solution of NH4CH3CO2 has a pH of approx 7. Explain this using two equations. I have one equation CH3COO-(aq) + H2O(l) --> CH3COOH(aq) + OH-(aq) What could the other equation be? NH4CH3CO2 is the salt of a weak acid and a weak base...
Friday, May 18, 2007 at 4:56am by Fiona

Chemistry
If a buffer solution is 0.190 M in a weak acid (Ka = 5.8 x 10^-5) and 0.550 M in its conjugate base, what is the pH? What if it said "if a buffer solution is ___ M in a weak base (Kb = ____) and ___ M in its conjugate acid, what is the pH? Would the steps from the first ...
Sunday, April 22, 2012 at 5:17pm by Katherine

Chemistry
CH3COOH + H2O = CH3COO- + H3O+ Acid acetic is a weak acid so not all of it will dissociate. The constant for acid acetic is 1.8 . 10^-5 therefore 1.8x10^-5=(x^2)/(0.2-x) x is the amount that disociated solve the equation and x is 1.88x10^-3 pH=-log(pH)=-log(1.88x10^-3)=2.72
Sunday, January 23, 2011 at 1:38pm by Tom

chemistry
I assume these are two separate solutions; i.e., two separate problems. The pH of the NH4ClO4 solution is determined by the hydrolysis of the salt. NH4ClO4 is the salt of a weak base (NH3) and a strong acid (HClO4), therefore, the NH4^+ is hydrolyzed. NH4^+ + HOH ==> NH3 + ...
Saturday, April 18, 2009 at 3:05pm by DrBob222

Chemistry- Acids and Buffers
Cyanic Acid is a weak acid HOCN + H2O <--> H3O+ +OCN- ka= 3.5*10^-4 a) if 2.5ml of 0.01 M cyanic acid solution is added to 25.0 ml of a formis acid buffer with ph = 3.70, what is the ratio of [OCN-]/[HOCN] in the resulting solution? b) determine the pH of a 0.500 M ...
Monday, April 9, 2012 at 4:21am by Tasneem

chemistry
For the weak acid HX, what is the pH of a 0.10 M solution if the acid is 4.0% ionized?
Sunday, November 28, 2010 at 11:36pm by cs

Chemistry
For the weak acid HX, what is the pH of a 0.10 M solution if the acid is 4.0% ionized?
Monday, February 21, 2011 at 11:19pm by JC

Chemistry 2
The pH of a 0.175 M aqueous solution of a weak acid is 3.52. What is Ka for this acid ?
Wednesday, September 22, 2010 at 9:31pm by Sammie

chemistry
The pH of a 0.175 M aqueous solution of a weak acid is 3.52. What is Ka for this acid ?
Friday, September 24, 2010 at 4:43pm by Anonymous

Chemistry
If the Ka of a monoprotic weak acid is 4.3*10^-6, what is the pH of a 0.16 M solution of this acid?
Sunday, July 24, 2011 at 12:35am by Josh

Chemistry
If the Ka of a monoprotic weak acid is 9.0 10-6, what is the pH of a 0.26 M solution of this acid?
Tuesday, October 25, 2011 at 8:39pm by Sevy

Chemistry/pH- Weak Acid
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 pH of 4.000. What volume of water must be added to make the pH = 5.000? My Calculations: To calculate the concentration of x, I take the pH value -&...
Sunday, August 17, 2008 at 6:01am by Mary

chemistry
oh This is an acid base experiment this is the last stage. There are two parts: part 1) 0.3470g sodium acetate trihydate is added to 15.00 ml acetic acid (concentration is 0.20) then its mixed and a ph is taking--i got 4.30 PH part II) Added 0.7618 g of sodium acetate ...
Thursday, July 16, 2009 at 7:35pm by Jim_R

Chemistry
A 0.10 M solution of a weak acid has a pH of 3.5 at 25%C. What is the equilibrium constant, Ka, for this acid?
Sunday, October 10, 2010 at 10:03am by Tara

chemistry
A 0.040M solution of a weak acid has a pH of 3.02 at 25C . What is the value of Ka for the acid?
Tuesday, March 15, 2011 at 11:11pm by darren

Chemistry
If an equal number of moles of the weak acid HOCN and the strong base KOH are added to water, the resulting solution will be acidic, basic or neutral? There is a complicated answer and a sensible answer. Both arrive at the same answer. But here is the logic for the sensible--I...
Friday, April 27, 2007 at 2:58pm by Joel

chemistry
hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M NaOH Base (in mL) is ...
Monday, July 12, 2010 at 3:05am by THOMAS

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
Saturday, April 5, 2008 at 6:37pm by Geroge B.

chemistry
What is the pH of a solution that is .200M in acid and .500 m in the corresponding salt if the weak acid ka= 5.0x10^-7
Thursday, September 2, 2010 at 11:07am by Rae

Chemistry
A weak acid solution, HX 0.37 M, has a pH of 3.70. Calculate the acidity constant for this acid.
Sunday, May 13, 2012 at 10:32pm by Andrea

chemistry
Ascorbic acid is a weak organic acid also known as vitamin C. A student prepares a 0.20 mol/L aqueous solution of ascorbic acid and measures its pH as 2.40. Based on this evidence, what is the Ka of ascorbic acid?
Sunday, April 6, 2008 at 12:46am by Laura

Chemistry
A 5.55g sample of a weak acid with Ka=1.3 x10^-4 was combined with 5.00 mL of 6.00 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.25. What is the molar mass of the weak acid?
Saturday, April 23, 2011 at 9:21pm by Trista Nigh

Chemistry(Please help, thank you!!)
Acid- Base titration of a weak-acid. H2S04 is a weak acid. NaOH is a strong base. pH = 14 + log(sqrt)[(M1*M2*Kw)/([M1+M2]*Ka)] M1 = Concentration of Weak Acid. M2 = Concentration of Strong Base. Kw = dissociation constant for water. Ka = dissociation constant for acid. Note: M...
Tuesday, October 25, 2011 at 10:21pm by Hurrrdurrbeedooda

Chemistry
Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is added to the buffer solution. 3) The pH of a ...
Monday, September 23, 2013 at 11:06pm by Aria

Chemistry
Thanks for poiting that out. I got a pH of 9.03. My only question is why the pH isn't acidic if it is a strong acid mixed with a weak base?
Tuesday, May 12, 2009 at 8:56pm by Chelsea

Chemistry
When diluting a weak acid and a strong acid, why is it that the pH changes more significantly in the strong acid? (consider the equilibrium occurring) With HCl
Saturday, March 13, 2010 at 12:42pm by Anonymous

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
The pH of a 0.010 M aqueous solution of a weak monoprotic acid, HX, is 4.5. What is the value of the acid ionization constant?
Thursday, May 17, 2012 at 12:16pm by Anonymous

Chemistry
Boric acid is a weak acid with an equilibruim constant(K)of 10-9.3. What is the pH balance of a 0.1 molar solution of boric acid?
Monday, October 8, 2012 at 12:01pm by Kenneth

chemistry
Lactic acid is a weak monoprotic acid. If a 0.10 M solution of it has a pH of 2.44, what is the dissociation constant (Ka) for lactic acid. I got 1.3x10^-4? Is that right?
Monday, October 3, 2011 at 5:46pm by person

Chemistry
i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=210-3 or one with Ka=810-6 c. a 0.1 M solutions of a base with pKb=4.5 or...
Saturday, April 6, 2013 at 3:08pm by m

Chemistry
i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=210-3 or one with Ka=810-6 c. a 0.1 M solutions of a base with pKb=4.5 or...
Saturday, April 6, 2013 at 9:24pm by m

Chemistry
i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=210-3 or one with Ka=810-6 c. a 0.1 M solutions of a base with pKb=4.5 or...
Sunday, April 7, 2013 at 7:47am by m

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