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April 20, 2014

Search: titrated

Number of results: 864

Chemistry
Calculate the concentration of a 50.0mL sample of HBr acid, which was titrated with 37.7 mL of 0.57 M NaOH base. Why is an overshot endpoint not a good titration?
Thursday, April 10, 2008 at 4:21pm by Jared

chemistry
A 0.446g sample of an unknown monoprotic acid was titrated with 0.105M KOH the molar mass is 120g/mol. What is the PKA value Who helps me to solve it for me. Please help
Saturday, August 4, 2012 at 10:31pm by Fai

chemistry
A 0.446g sample of an unknown monoproctic acid was titrated with 0.105 M KOH The molar mass is 120g/mol. What is the PKA value? Pls helps me again
Sunday, August 19, 2012 at 12:35am by Fai

chemistry
thanks, sorry, 10ml of the unknown mixture was titrated methyl orange was used it took 7.5ml of 1M HCl (.0074Mol ?) so this means .00074Mol CH3NH2 / ml ?
Friday, August 24, 2012 at 8:05pm by jeffrey

chemistry
When 50.0 mL of 0.050 M formic acid, HCHO2, is titrated with 0.050 M sodium hydroxide, what is the pH at the equivalence point?
Wednesday, April 11, 2012 at 6:02am by chamy

CHEM
IF A 50.0 ML SAMPLE OF CALCIUM HYDROXIDE IS TITRATED WITH 25.0 ML OF 0.200M PHOSPHORIC ACID, WHAT IS THE MOLARITY OF THE BASE?
Tuesday, May 7, 2013 at 1:14pm by SHANNA

Chemistry
what is important about oxygen being formed during a titration?? (formed in container after it has been titrated not in the burette)
Tuesday, October 29, 2013 at 5:06pm by Amber

Chemistry
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....? A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP, with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and a final buret ...
Wednesday, March 7, 2012 at 3:58pm by Cynthia

chemistry
25.0g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?
Friday, May 28, 2010 at 8:38pm by Cynthia

chemistry
21.00 mL of 0.200 M HBr is titrated with 0.351 M NaOH. What is the pH after the addition of 6.56 mL of the base ?
Friday, November 5, 2010 at 3:14am by lizz

chemistry
A 25 mL solution of .5M NaOH is titrated until neutralization into a 50mL sample of HCl. What was the concentration of HCl?
Tuesday, February 22, 2011 at 10:56pm by E

CHEMISTRRY
what is the molarity of an H2SO4 solution if 49.0 ml is completely titrated by 68.4ml of an NaOH solution whose concentration is 0.333 M?
Tuesday, June 8, 2010 at 3:34pm by George

chemistry
if 50.0 mLs of HCl of unknown concentration is titrated to neutrality with 90.0 mL of .650 M NaOH. calculate the molarity of the HCl
Monday, November 14, 2011 at 5:15pm by susan

chemistry
if 50.0 mLs of HCl of unknown concentration is titrated to neutrality with 90.0 mL of .650 M NaOH. calculate the molarity of the HCl
Monday, November 14, 2011 at 5:15pm by susan

chemistry
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
Monday, March 19, 2012 at 3:28pm by Sharnam

chemistry
25mL of tartaric acid solution is titrated against 31mL of NH4OH. What is the normality of the NH4OH? Please explain how to work this problem.
Friday, October 5, 2012 at 1:15pm by Stephen

Chemistry
50.0 mL of 0.116 M NaOH is titrated with 0.0750 M HCl. Calculate the pH after the addition of 5.0 mL volume of acid.
Wednesday, May 1, 2013 at 12:33am by Nathan

chemistry
Using a BCA table, calculate the molarity of a 25.0 mL sample of HNO3 thats is titrated to its endpoint with 22.7 mL of 0.200 M NaOH.
Sunday, May 11, 2008 at 12:25pm by caleb

Chemistry
How many mL of 0.139 M KOH are needed to reach the equivalence point when 1.8 g of potassium hydrogen phthalate, KHP is titrated to a phenolphthalein end-point.
Sunday, October 9, 2011 at 10:21pm by Anonymous

Chemistry
How many mL of 0.139 M KOH are needed to reach the equivalence point when 1.8 g of potassium hydrogen phthalate, KHP is titrated to a phenolphthalein end-point.
Sunday, October 9, 2011 at 10:24pm by Anonymous

Physical chemistry 2
50 ml of 0.02M acetic acid is titrated with 0.1M NaOH.Calculate the pH of the solution when 10ml of NaOH is added
Tuesday, March 12, 2013 at 12:41am by Anonymous

chemistry
to get the grams of NaClO in the titrated bleach sample I calculated .000721 x 74.44217 = .0536 which was correct. For the previous question I asked I put in the same answer as you said and it is incorrect.
Sunday, October 27, 2013 at 9:38pm by Morgan

Chem
Find and show work the final pH when 35mL of 0.200 mol/l sulfuric acid are titrated with 18mL of 0.030 mol/L sodium hydroxide?
Wednesday, May 26, 2010 at 8:13pm by S.S

Chemistry
Can someone please explain me how to do this problem? A 25mL solution of 0.5 M NaOH is titrated until neutralization into a 50mL sample of HCl. What was the concentration of the HCl?
Thursday, February 24, 2011 at 12:58pm by Abigail

chemistry
What chemical reaction is responsible for the endpoint observed when the NH3/NH4Cl buffer solution is titrated with HCl? Write a blanced ionic equation for the reaction.
Sunday, March 27, 2011 at 7:21pm by redgy

chemistry
a 30.0ml sample of diprotic acid is titrated with .260M KOH. if 68.5ml is required to reach the equivalence point, what is the concentration of the acid?
Wednesday, October 12, 2011 at 4:12am by john

Chemistry
if 20 ml of Formic acid is combined with 30 ml of distilled water and titrated with .10 M NaOH. What is the theoretical endpoint (equivalence point)
Tuesday, October 18, 2011 at 7:50pm by Jenna

Chemistry
A 100.0 ml sample of .50 M HCl (aq) is titrated with a .10 M NaOH. What volume of the NaOH solution is required to reach the endpoint of the titration?
Tuesday, March 13, 2012 at 1:02am by Arianna

Chemistry
You don't provide enough information for me to know what you did. Did you titrated with H2O2? If so you knew the molarity and that's all you needed. Were you titrating bleach? You wanted to know % w/w and for that you had to know the mass of the bleach solution?
Sunday, October 28, 2012 at 10:56pm by DrBob222

chemistry
You're post is too sketchy. For example, did you add KI to the bleach to free up I2 and the I2 was titrated with thiosulfate? Of did you use some other procedure.
Sunday, October 27, 2013 at 9:38pm by DrBob222

chemistry
I have no idea what concn is being titrated in Fig 17-9; however, if we consider it 100 mL of 0.1M HCl being titrated with 0.1M NaOH, we can ESTIMATE it this way. You start with 0.1M and you want the concn of H^+ to be 0.01 (pH of 2) at the end; therefore, the concn must be ...
Thursday, April 14, 2011 at 8:17am by DrBob222

chem help w/ Lab
Weight of the mustard package Sample: 3.02 (g) Weight of the mustard package Solution: 33.3 (g) Trial #1 Trial #2 Trial #3 Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909 Weight of NaOH Solution Delivered (g) : .354 .304 .269 Concentration of NaOH : 7.48e-3 (...
Wednesday, October 17, 2012 at 3:19am by Den

chemistry
When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks
Thursday, March 25, 2010 at 1:24am by josh

chemistry
predict the pH of the solution obtained when a 1.0 M magnesium hydroxide solution is titrated with an equal amount of a 1.0 M solution of sodium chloride.
Monday, March 29, 2010 at 5:45pm by Ash

chem help
if 20 ml of .025M Formic acid is combined with 30 ml of distilled water and titrated with .10 M NaOH. What is the theoretical endpoint (equivalence point)
Wednesday, October 19, 2011 at 10:16am by Jenna

Chemistry
25.0 ml of a 0.100 M solution of the weak acid, CH3OOH is titrated with a 0.10 M solution of the strong base, NaOH. Calculate the pH of the equivalence point.
Sunday, February 26, 2012 at 10:44am by ASood

Chemistry
a 0.451 L solution of 1.71 ascorbic acid (ka1=7.9E-5, ka2=1.6E-12) is titrated with 1.35 M NaOH. What is pH when 0.9540 L of NaOH is added?
Tuesday, December 11, 2012 at 3:30pm by Chris

Chemistry
A 17.6ml sample of a monoprotic acid is titrated with 0.212M NaOH. If 69.2ml of base is required to reach the equivalence point, what is the concentration of the acid?
Friday, April 19, 2013 at 12:56am by Chloe

chemistry
calculate the pH of the solution when 25.0ml of 0.0920M HCL is titrated with 0.15ml, 23.0ml, 30.0ml of 0.10M NaOH
Wednesday, January 23, 2013 at 12:08pm by nathalie

analytical chemistry
When a monoprotic weak acid is titrated with a strong base, the titration curve contains these many inflection points: a.zero b.one c.two d.three Can you also explain why you choose your answer to this question...thanks
Wednesday, March 24, 2010 at 6:35pm by josh

Chemistry Lab
The only thing I can suggest is to use the numbers you have, assume that is the end point, and calculate the amount of Zn in your sample. Then weigh an amount of Zn or Zn salt equal to the amount you have calculated as being in your sample, add the same materials as you did to...
Monday, November 10, 2008 at 3:41pm by DrBob222

chemistry
There must be more to it than that. NaOCl can't be titrated with thiosulfate, at least not when I went to school. The USUAL process is to treat a solution of bleach with KI and titrate the liberated I2 with thiosulfate.
Wednesday, November 3, 2010 at 6:16pm by DrBob222

Chemistry
I was just wondering how I would determine the pKb of a weak base that was titrated with a strong acid on a titration curve at the EQUIVALENCE POINT. And from this, how would I find the pH? PLEASE HELP!!
Thursday, March 28, 2013 at 8:56pm by TC

chemistry
one last question. From same set up. Assuming all of the hypochlorite ion comes from sodium hypochlorite, calculate the grams of NaClO in the titrated bleach sample.
Sunday, October 27, 2013 at 9:38pm by Morgan

chemistry
I know the formula is Ma x Mla / 1000 x Sa / Sb = Mb x Mlb / 1000 if 175 ml of KOH of unknown concentration with a methyl red indicator present is titrated with [0.275 M] H3PO4, the yellow solution turns red after 29.6 ml of the H3PO4 is added. What is the molarity of the KOH...
Thursday, September 4, 2008 at 9:14am by casey

Chemistry
Can anyone answer this question please. (Determine the concentration of an aqueous NaCl solution if 31.5 mL are required to reach the equivalence point when titrated with 25.0 mL of 0.20 M AgNO3.)
Sunday, September 19, 2010 at 10:23pm by John

Chemistry
A 23.0mL sample of a diprotic acid is titrated with 0.260M KOH. If 55.5mL of base is required to reach the second equivalence point, what is the concentration of the acid? I'm not sure how to do this.
Sunday, February 6, 2011 at 7:18pm by Melissa

Chemistry
A solution of K2CrO4 was titrated with AgNO3, using a silver indicator electrode (E=0.799V) and a S.C.E. electrode (E=0.241V). The product, Ag2CrO4, has a Ksp = 1.1x10^-12. What is the potential at the equivalence point?
Monday, May 28, 2012 at 7:43pm by Jeanie

Balthazar
A 30 ml sample of of 0.150 m hydrazoic acid (ka = 4.50x10^-4 ) is titrated with a 0.100 m NaOH what is the ph after the ff additions of NaOH 30ml 45ml 60ml
Thursday, August 1, 2013 at 2:09pm by Omi

Chemistry
100 mL of 1.0 M formic acid (HCOOH) is titrated with 1.0 M sodium hydroxide (NaOh). The Approximate pKa is 4 At the pKa, what fraction of the carboxyl group will have been converted to COO-?
Friday, September 27, 2013 at 10:13pm by Aria

Chemistry
A 119.2mL sample of 0.105M methylamine (CH3NH2, Kb=3.7*10^-4) is titrated with 0.255M HNO3. Calculate the after the addition of each of the following volumes of acid. 49.1mL and 73.6mL. Please help.
Sunday, February 6, 2011 at 7:23pm by Melissa

chemistry
what is the molarity of a sodium hydroxide solution if 26.0mL of the solution os titrated to the end point with 57.5mL of a 0.500M hydrochloric acid solution
Friday, March 8, 2013 at 11:50am by casey

Science
What is the pH of 115 mL of a 1.50 m solution of HNO2 that is titrated with a 1.50 M solution of LiOH at the equivelence point?
Wednesday, June 20, 2012 at 2:27am by Jake

chemistry
25 milliliters of tartaric acid solution is titrated against 31 milliliters of NH4OH. What is the normality of the NH4OH?
Wednesday, October 3, 2012 at 6:10pm by Stephen

Chemistry
What is the pH of a solution of 40.0 ml of 0.800 M HCl titrated with 4.00 ml of 1.00 M Hydroxyl amine?
Wednesday, April 24, 2013 at 10:43pm by Sara

chemistry
What is the molarity of an unknown acid if 40.5 ml of the acid can be titrated to an end point by 20.5 ml of 0.2250 M NaOH?
Saturday, October 16, 2010 at 5:54pm by bev

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
Thursday, November 11, 2010 at 2:29am by flame

chemistry
When 25ml of 0.10 mol/l HBr is titrated with 0.10 mol/l NaOH, what is the pH at the equivalence point?
Tuesday, June 15, 2010 at 4:19pm by Adeola

chemistry
A 35.0 ml sample of 0.225 M HBr was titrated with 42.3 ml of KOH. What is the concentration of the KOH?
Monday, December 5, 2011 at 2:21pm by Anonymous

Chemistry
A 35.0 ml sample of 0.225 m HBr was titrated with 42.3 ml of KOH. What is the concentration of the KOH
Tuesday, December 6, 2011 at 10:43pm by Anonymous

CHEMISTRRY
What is the molarity of an HCl solution if 49.0 mL is completely titrated by 68.4 mL of an NaOh solution whose concentration is 0.333 M?
Tuesday, June 8, 2010 at 3:34pm by Mel

Chemistry
What is the pH when 25 mL of .20 M CH3COOH has been titrated with 35 mL of .10 M NaOH? I got the answer .0375 but that is incorrect if you could show me steps maybe i can figure out what i did wrong thanks
Tuesday, November 30, 2010 at 10:09pm by Mya

chem 2
I just need help setting up this equation. NH3 is titrated with HCL. Does this mean the reaction is this? NH3 + HCL --> NH4 + CL- ??
Monday, July 6, 2009 at 12:32am by Anonymous

Chemistry
A 80.0 mL volume of 0.25 M HBr is titrated with 0.50M KOH. Calculate the pH after addition of 40.0 mL of KOH.
Thursday, July 16, 2009 at 4:35pm by Saira

Chemistry
A 80.0 mL volume of 0.25 M HBr is titrated with 0.50M KOH. Calculate the pH after addition of 40.0 mL of KOH.
Thursday, July 16, 2009 at 6:03pm by Saira

chemistry
0.25 g of acid is titrated with .108 M NaOH. if it takes 27.22 mL of NaOH to reach the endpoint, what is the equivalent weight of the acid?
Sunday, February 7, 2010 at 8:51pm by sean

chemistry
A 40 mL sample of 0.25 M NaCHOO is titrated with 0.2 M HCl. What is the pH of the solution after 140 mL of HCl has been added?
Wednesday, March 2, 2011 at 2:23pm by Eddy

chemistry
When a 0.5725 g sample of Lysol was titrated with 0.100 M NaOH, and endpoint was obtained at 15.00 mL. What is the percent of HCL in the lysol sample?
Monday, June 21, 2010 at 7:41pm by Alisha

Chemistry
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 ml of .75M sulfuric acid?
Wednesday, May 18, 2011 at 8:38pm by Christian

chemistry
When a 0.5725 g sample of Lysol was titrated with 0.100 M NaOH, an endpoint was obtained at 15.00 mL. What is the percent of HCl in the Lysol sample?
Thursday, March 22, 2012 at 10:22am by hank

Chemistry
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 mL of 0.75M sulfuric acid?
Tuesday, May 1, 2012 at 4:21pm by Emily

Chemistry
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 mL of 0.75M sulfuric acid?
Tuesday, May 1, 2012 at 4:40pm by Emily

chemistry
A volume of 100mL of a 0.800 M HNO3 solution is titrated with 0.640 M KOH. Calculate the volume of KOH required to reach the equivalence point.
Monday, August 6, 2012 at 7:13pm by LL

CHEM PROB MR BOB
Is the 7.7 right? All those assumptions I made in my answer yesterday still bother me. However, assuming you have checked a database and things are in order, then 2.35E-3 is right. The second number of 0.30 I would make 0.303 since you're allowed another place. For the last ...
Wednesday, October 10, 2012 at 3:14am by DrBob222

Chemisty
In titrations of acids and bases, what is the difference between the end point of the titration, and the equivalance point? Also, what is chemically occuring during the buffer zone? Thanks! Good question and one that students sometimes have trouble with. The equivalence point ...
Tuesday, May 15, 2007 at 9:47pm by Jessie

chemistry
25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L acetic acid. Calculate the pH of the solution
Wednesday, April 9, 2008 at 9:26pm by unknown

chemistry
A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________.
Tuesday, July 24, 2012 at 10:40pm by katie

Chemistry
"Find the pH of the solution obtained when 32 mL of 0.087 M ethylamine is titrated to the equivalence point with 0.15 M HCl? Do I need to do a rice table for this problem? I'm having difficulty starting this problem... Thanks!
Monday, May 21, 2007 at 5:42pm by Rachel

Chemistry
A 30.00ml sample of 0.1234 M hypobromous acid (HBrO) is titrated with a 0.2555 M KOH solution. The Ka for HBrO is 2.5*10^-9 Calculate the pH of teh titration mixture at the equivalence point.
Saturday, April 17, 2010 at 11:28am by Anonymous

chemistry
A volume of 40.0 of aqueous potassium hydroxide was titrated against a standard solution of sulfuric acid h2so4. What was the molarity of the solution if 20.02 of 1.50M h2s04 was needed? Who helps me to solve it for me.
Tuesday, July 31, 2012 at 11:44pm by Fai

Chemistry
A solution consisting of 25.00 g Nh4Cl in 178 ml of water is titrated with 0.114M KOH. How many mL of KOH are required to reach the equivalence pt?
Thursday, March 24, 2011 at 9:04pm by Ashley

chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
Wednesday, April 20, 2011 at 1:11pm by Mike

chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
Wednesday, April 20, 2011 at 1:23pm by Mike

chemistry
31.0mL sample of LiOH, concentration unknown, is titrated with .52 M HCl. It takes 42.9 ml of HCl to reach the endpoint. What is the concentration of the base?
Thursday, April 26, 2012 at 11:35pm by kendra

Chem
A 75.0 mL volume of 0.200 M NH3 (Kb=1.8x10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 28.0 mL of HNO3.
Wednesday, April 2, 2014 at 12:43am by Billy Bob Reynolds

chemistry
Cu(II) reacts with I^- to produce CuI, a ppt, and liberates I2. The I2 is titrated with thiosulfate. Left on its own, the excess I^- from the KI can be oxidized by air to give more I2.
Thursday, January 31, 2008 at 11:41am by DrBob222

chem
help, i'd like to know how to do this titration question: for example: a 1g sample of naoh contaminated with na2co3 is titrated with 0.500MHCl, and it is found that 46.5mL of HCl are required for neutralization. Find the percentage by mass Na2Co3. thank you in advance
Sunday, April 20, 2008 at 11:06pm by Alex

chem class
A 25.00-mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is ???? M.
Tuesday, November 23, 2010 at 11:23pm by richard

Chemistry
A 25 mL sample of wine is found to have a concentration of acetic acid of 0.23 M. If this was titrated with a 0.16 M NaOH solution how many mL's of NaOH would be required?
Saturday, November 27, 2010 at 5:44pm by Susan

chemistry
which of the following was not one of the products when you titrated the vinegar solution with sodium hydroxide? HC2H3O2+NaOH===>NaC2H3O2+H2O a salt water sodium acetate acetic hydroxide
Tuesday, July 13, 2010 at 4:05pm by Anonymous

chem
A sample of potassium hydrogen oxalate, KHC204, weighing 0.717 g, was dissolved in water and titrated with 18.47 mL of an NaOH solution. Calculate the molarity of the NaOH solution.
Wednesday, November 21, 2012 at 2:52pm by amanda78

College Chemistry
Calculate the pH at the equivalence point if 25.00 mL of 0.010M barbituric acid (HC4H3N2O3) is titrated with 0.020M NaOH. (Ka barbituric acid = 1.0 x 10^-5)
Tuesday, July 9, 2013 at 2:03pm by Mary

chemistry
You don't have questions here. Mostly just statements. Here is the equation. HA + NaOH ==> H2O + NaA I assume the benzoic acid was titrated with the NaOH and the question is to determine the molar mass of benzoic acid. LNaOH x M NaOH (from part a) = moles NaOH. moles HA = ...
Friday, November 4, 2011 at 1:19am by DrBob222

chem
a solution of weak acid of molarity 0.05 mol/dm3 is titrated against 0.1mol/dm3 NaOH, the pka = 3.67 what volume of acid would u use in ur titration?
Sunday, December 7, 2008 at 10:45pm by Kimora

Chemistry
A 50.0 mL sample of 0.23 M propanoic acid, CH3CH2COOH, a weak monoprotic acid, is titrated with 0.14 M KOH. Ka of CH3CH2COOH = 1.4 multiplied by 10-5. What is the pH at equivalence point?
Sunday, April 3, 2011 at 5:10pm by George

Chemistry
you have 20 ml of 0.1 M aqueous solution of the weak base (CH3)N (Kb = 7.4 x 10^-5). This solution will be titrated with 0.1 M HCl. how many ml of acid must be added to reach the equivalence point?
Wednesday, February 8, 2012 at 6:17pm by laura

Chemistry
A 0.5224g sample of an unknown monoprotic acid was titrated with 0.0998M of NaOH. The equivalence point of the titration occurs at 23.82 mL. Determine the molar mass of the unknown acid.
Sunday, April 29, 2012 at 9:42pm by Confused

chemistry
formic acid is a monoprotic acid with a ka at ml solutionof m of formic acid solution is titrated with m naoh what is the ph at the equivalence point
Tuesday, March 29, 2011 at 8:07pm by Omar

Science
A 10 mL sample of tartaric acid (a diprotic acid) is titrated with 20 mL of 1.0 M NaOH. What is the molarity of the acid?
Thursday, December 29, 2011 at 7:20am by Fahmi

chemistry
What is the molarity of an HCl solution if 14.0mL HCl solution is titrated with 22.6mL of 0.155 M NaOH solution?
Saturday, February 9, 2013 at 2:04pm by Peter

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