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April 20, 2014

Search: diluted pH

Number of results: 7,508

Biochemistry
An acid diluted DOES change the pH. A base diluted DOES change the pH. For example, 0.1 M HCl has a pH of 1. Dilute that by a factor of 2 and the concn = 0.05. The pH of that solution is -log(0.05) = 1.30
Friday, June 24, 2011 at 12:47am by DrBob222

chemistry
pH = -log(H^+). Plug in 3.00 for pH and calculate (H^+). Since the solution is diluted by a factor of two, then (H^+) in the diluted solution will be 1/2 of the initial value. Plug in the new (H^+) and solve for the new pH. Hint: it will NOT be 1/2 of 3.00.
Tuesday, May 5, 2009 at 11:06pm by DrBob222

chemistry
An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. Wht is the pH of the diluted solution?
Tuesday, May 5, 2009 at 11:06pm by j

chemistry
Aqueous solution with a pH of 10.6 is diluted from 1 L to 1.5 L. What is the pH of the diluted solution?
Sunday, March 14, 2010 at 6:39pm by elizabeth

Chem Webwork
Complete the table below: What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water (like it will be in the experiment you perform in lab)? mL NaOH: 0.70 pH w/ HCl: 2.14 pH w/ HC2H3O2: ??? I got pH w/ HCl, but I can'...
Monday, April 25, 2011 at 4:25pm by Michelle

Chemistry DrBob
What is the pH of the solution created by combining 2.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 2.30 ________ _________ What are the pH values if you take into account that the 8.00 mL ...
Thursday, May 1, 2008 at 4:53pm by Amy

Chemistry
A). The pH of PURE water is 7.0. Distilled water CAN be less than 7.0 if it has absorbed some CO2 from the air. B) The 6.0 M HCl has been diluted 1 mL to 41 mL; therefore, molarity of HCl is 6.0 x (1/41) = ??. HCl is a strong electrolyte and ionizes 100%; therefore, the H^+ is...
Thursday, November 1, 2007 at 9:35pm by DrBob222

Chemistry
mL x M = mL x M Solve for the M of the diluted HCl, then plug into the pH equation. Then pH = -log(H^+) = ??
Wednesday, April 6, 2011 at 6:14pm by DrBob222

Chemistry
first dilution: you diluted it to 10/19 of .1M, so it is 10/190 M. Then you diluted it 10/100 of its concentration, new concentration 10/1900 M the statement <The student diluted the sample as above 1 time(s).>> makes no sense to me, it it means my first paragraph, ...
Monday, April 7, 2014 at 5:13pm by bobpursley

Chem Webwork help
1. What is the pH when enough 0.10 M Base (in mL) is added to neutralize 8 mL of 0.10 M Acid? Complete the following table. NaOH HC2H3O2 2. What is the pH of the solution created by combining 2.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of ...
Monday, July 12, 2010 at 2:34am by Sammy

Chemistry
(HBr) diluted = 0.000625 x (146.6/860) = about 1.08E-4 pH = -log(H^+) = -log(HBr) since HBr is a strong acid and ionizes 100%. Then pH + pOH = pKw = 14. You know pH and pKw solve for pOH.
Thursday, March 21, 2013 at 1:37am by DrBob222

chemistry
What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water? This is in regards to my previous question. We are still calculating the pH of w/HCl and w/HC2H3O2. I don't really understand what to do with the 100ml.
Sunday, July 11, 2010 at 10:44pm by Sara

Chemistry -- to Dr.Bob
I know this convo happened a while ago lol. but i seriously don't know how to find the HCL pH for this: What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water
Friday, May 2, 2008 at 9:41pm by Help!

Chemistry, Urgent!
You need to be aware that the HF is a weak acid and ionizes only partially with a Ka of about 7.2 x 10^-4 so the (H^+) contributed by the HF, in comparison to the 100% ionized HCl, is too small to count it. So the pH of the solution is essentially the pH of the HCl. You have ...
Thursday, February 26, 2009 at 12:20am by DrBob222

chemistry
how do you solve this What is the pH of the solution created by combining 2.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH 2.60 pH wHCl: _ pH wHC2H3O2 : _ Complete the table below: What are the pH values if you ...
Monday, July 12, 2010 at 6:03pm by Jin

CHEMISTRY (WEBWORK)
What is the pH of the solution created by combining 1.20 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH w/ HCl pH w/ HC2H3O2 1.20 ? ? Complete the table below: What are the pH values if you take into account ...
Monday, July 12, 2010 at 6:19pm by Anonymous

Physical Chem
A student added solid K2O to a 750.0 mL volumetric flask. The solid was dissolved in water and then the flask filled with water to the mark. This formed 750.0 mL of the initial KOH solution. 20.0 mL of the initial solution was transferred to another flask and diluted to 200.0 ...
Thursday, May 27, 2010 at 3:55am by Sara

Chemistry
A 200 mg/dl solution was diluted 1:10. This diluted solution was then additionally diluted 1:5. What us the concentration of the final dilution?
Tuesday, March 24, 2009 at 5:51pm by Jessi

chem lab (webwork)
What is the pH of the solution created by combining 1.80 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 1.80 Complete the table below: What are the pH values if you take into account that the 8....
Tuesday, April 13, 2010 at 9:36pm by anonymous

Chemistry
You need the molarity of HCl. You can take some liberties with the question in as much as it says completely neutralized. You can assume that you have 1 mL of 0.1M NaOH in excess which will be diluted to 0.10M x (1/21) = 0.00476 Then pOH = -log(OH^-), find pH from pH + pOH = ...
Tuesday, March 6, 2012 at 7:56pm by DrBob222

chemistry
What is the pH of the solution created by combining 12.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 12.30 What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was...
Monday, May 5, 2008 at 5:31am by Renee

Chemistry
One example each for 0.1M HCl/NaOH added to 25 mL H2O. The diluted HCl solution is 0.1M x (1 mL/26 mL) = (HCl) pH = -log(HCl) The diluted NaOH solution is 0.1M x (1 mL/26 mL) = (NaOH) pOH = -log(NaOH). Then pH + pOH = pKw = 14.00
Monday, March 14, 2011 at 9:32pm by DrBob222

Chem Webwork UCI
Complete the table below: What is the pH of the solution created by combining 0.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH: 0.70 pH w/ HCl: 1.08 pH wHC2H3O2: 3.23 Complete the table below: What are the pH ...
Monday, April 25, 2011 at 4:50pm by Michelle

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
calculate the pH of 20.00mL of 2.00 M HCl diluted to 0.500 L
Sunday, February 26, 2012 at 6:28pm by Colin

Chemistry
Given 3.90mL of 1.80M HCl diluted to .520L, whats the pH?
Thursday, April 5, 2012 at 7:07am by Alex

Chemistry
Given 3.90mL of 1.80M HCl diluted to .520L, whats the pH?
Thursday, April 5, 2012 at 8:05am by Alex

chemistry
how do you solve this? What is the pH of the solution created by combining 12.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 12.30 Complete the table below: What are the pH values if you take...
Monday, July 12, 2010 at 1:05am by Jin

chemistry
a buffer composed of 0.50mol acetic acid and 0.50mol sodium acetate is diluted to a volume of 1.0L. The pH of the buffer is 4.74. How many moles of NaOH must be added to the buffer solution to increase its pH to 5.74?
Wednesday, October 7, 2009 at 9:20pm by millie

chemistry
What volume of 12M HCl must be diluted to make 2L of solutioin with a pH of 4?
Sunday, April 25, 2010 at 9:39am by Anonymous

chemistry
What volume of 12 M HCL must be diluted to make 2L of solution with pH of 4?
Wednesday, April 28, 2010 at 10:46am by Anonymous

chemistry
HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid.
Tuesday, November 24, 2009 at 2:29pm by Anonymous

Chemistry!
HB, pH=1 To neutralize 10cm3 it took 5.00cm3 NaOH 10cm3 of the solution HB are diluted with water to make 1 litre of solution. The pH of the new solution is 3. Show that HB is the strongest acid.
Tuesday, November 24, 2009 at 5:53pm by Anonymous

Chemistry
What is the pH of the solution obtained when 125 mL of 0.614M NaOH is diluted to 16.0 L with water?
Tuesday, November 9, 2010 at 7:33pm by Jenna

Chemistry
What is the pH of the solution created by combining 12.20 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH w/HCl pH w/HC2H3O2 12.20 =================================== my work: 0.000420 moles of NaOH / 0.020 ...
Monday, May 3, 2010 at 2:50pm by Amphee

CHemistry
True/ False: The pH of a soln that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH soln Would it be true since CH3COOH and CH3COONa are both weak acids, and if you mix them together, it becomes more diluted, and hence should have a higher...
Monday, May 5, 2008 at 5:26pm by Stephanie

Chemistry
The 0.100 M HCl has been diluted from 10 mL to 20 mL; therefore, (HCl) = 0.100 x (10/20) = 0.05M pH = -log(H^+) pH = -log(0.0500) pH = -(-1.301) = 1.301
Sunday, June 12, 2011 at 12:01am by DrBob222

P. Chemistry
A student added solid K2O to a 750.0 mL volumetric flask. The solid was dissolved in water and then the flask filled with water to the mark. This formed 750.0 mL of the initial KOH solution. 20.0 mL of the initial solution was transferred to another flask and diluted to 200.0 ...
Tuesday, February 23, 2010 at 5:32pm by Mark

chemistry
The pH of saturated is found to be 13.12. A 15.0mL sample of saturated Sr(OH)2 is diluted to 250.0mL in a volumetric flask. A 15.0 mL sample of the diluted Sr(OH)2 is transferred to a beaker, and some water is added. The resulting solution requires 27.6mL of a HCl solution for...
Monday, April 11, 2011 at 5:04am by chips ahoy

Chemistry
If a 0.1 mol/L solution is diluted to 0.01 mol/L, the: a) concentration of hydrogen ions increases b) pH decreases c) acidity constant decreases d) the acidity constant does not change I would think the ph decreases? no?
Monday, May 20, 2013 at 2:58pm by scilover

chemistry
Disadvantage of using pH indicators for what? For titrations it is that not all indicators change at the equivalence point pH. If for determining the pH of a solution, it is because most pH indicators have a pH range of about 2 pH units which isn't very close if you want to ...
Wednesday, April 29, 2009 at 8:23pm by DrBob222

CHEMISTRY FOR DR. BOB or anyone else
A hypothetical weak acid HA, was combined with NaOH in the following proportions: 0.20 mol HA, 0.08 mol NaOH. The mixture was then diluted to a total volume of 1L, and the pH measured. (a) If pH=4.80, what is the pKa of the acid (b) how many additional moles of NaOH should be ...
Friday, May 11, 2007 at 12:39pm by Delli

chemistry
A strong acid solution with H+=4 is diluted to twice its original volume. Will the pH go up, down, or stay the same?
Sunday, April 25, 2010 at 1:24pm by Anonymous

Chemistry
What is the pH of the solution created by combining 12.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH:12.30 pH w/ HCl _________ pH w/ HC2H3O2 _________ What are the pH values if you take into account that the 8....
Sunday, April 29, 2012 at 3:20am by HELP!!

Chemistry
What is the pH of the solution created by combining 12.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH:12.30 pH w/ HCl _________ pH w/ HC2H3O2 _________ What are the pH values if you take into account that the 8....
Sunday, April 29, 2012 at 3:21am by HELP!!

chem
The pH of saturated Sr(OH)2 is found to be 13.12. A 15.0ml sample of saturated Sr(OH)2 is diluted to 250.0ml in a volumetric flask. A 15.0ml sample of the diluted Sr(OH)2 is transferred to a beaker, and some water is added. The resulting solution requires 29.3ml of a HCl ...
Thursday, April 2, 2009 at 12:13pm by tomi

chem lab (webwork)
What is the pH of the solution created by combining 1.80 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH pH wHCl pH wHC2H3O2 1.80 Complete the table below: What are the pH values if you take into account that the 8....
Thursday, April 15, 2010 at 11:05pm by anonymous

Chemistry
1. What is the pH of the solution created by combining 0.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? 2. What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of...
Monday, November 1, 2010 at 12:14am by Kyo

CHEMISTRY FOR DR. BOB or anyone else
A hypothetical weak acid HA, was combined with NaOH in the following proportions: 0.20 mol HA, 0.08 mol NaOH. The mixture was then diluted to a total volume of 1L, and the pH measured. (a) If pH=4.80, what is the pKa of the acid (b) how many additional moles of NaOH should be ...
Friday, May 11, 2007 at 12:38pm by Delli

Science
5.00 ml of 1.90M HCl is diluted to 0.400l. calculate the pH of the HCl?
Tuesday, September 25, 2012 at 9:30pm by Erik

Science
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 4:25pm by DrewS

Chemistry
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 7:26pm by DrewS

Chemistry
Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 8:09pm by norma

chem
I got part 1: What is the pH of the solution created by combining 1.10 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? pH w/HCl =1.12 w/HC2H3O2(aq)= 3.94 But how do you do part two? What are the pH values if you take into ...
Thursday, April 29, 2010 at 12:13am by Adam

Chemistry
What is the pH of the solution created by combining 2.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water...
Monday, May 3, 2010 at 3:37pm by Ashley

Chemistry
What is the pH of the solution created by combining 2.70 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water...
Monday, May 3, 2010 at 3:37pm by Ashley

Chemistry
Okay, so based on the chart in my book I was able to determine the following. pH=(unknown) pKa=7.2 of Phosphoric Acid (2) A-=.5M of Na2HPO4 HA=.3M H2PO4- pH= 7.2 + log(.5/.3) pH=7.2+log(1.6667) pH=7.2+0.5108 So, the pH of this solution is: pH=7.7108 Correct?
Wednesday, July 6, 2011 at 11:13am by Shaun

chemistry
you diluted it first by a facator of 5 (2ml to 10 ml). then you diluted it by factors of 3. dilution: 5*3*3=45 times
Tuesday, September 13, 2011 at 8:27pm by bobpursley

Chemistry
Calculate [OH-] and pH for the following strong base solution: 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL
Monday, April 18, 2011 at 7:52pm by Kendall

Chem
Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What is the pH of the solution created by combining 1.90 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? mL NaOH: 1.90 pH w/HCl...
Monday, May 7, 2012 at 1:07pm by Jenna

chemistry
The pH of saturated Sr(OH)2 (aq) is found to be 13.12. A 10.0 mL sample of saturated Sr(OH)2 (aq) is diluted to 250.0 mL in a volumetric flask. A 10.0 mL sample of the diluted Sr(OH)2 (aq) is transferred to a beaker, and some water is added. The resulting solution requires 26....
Sunday, March 28, 2010 at 5:41am by anonymous

Science
a. (H^+)(OH^-) = Kw -= 1E-14 b. X = pH of 5; Y = pH of 4. c. pH = -log(H^+) Solve for (H^+)l. d. pH < 7 = acid pH = 7 = neutral pH > 7 = basic e. See b and d. f. pH + pOH = pKw = 14; then pOH = -log(OH^-)
Monday, September 10, 2012 at 1:03pm by DrBob222

chemistry
Calculate pH for strong base solution: 15.0 mL of 1.2010^−2 M Ca(OH)2 diluted to 460.0 mL
Sunday, February 26, 2012 at 6:49pm by jeff

Chemistry
Hi, I'm a little stuck on this problem: Find the pH of the Hydrochloric acid solution when 5.0 mL of concentrated HCl, with a specific gravity of 1.18 and has 37% (w/w) purity is diluted to 2.0L
Monday, November 11, 2013 at 8:08pm by T

chemistry
The urine excreted by an adult patient over 24 hours was collected and diluted to give 2.000L sample. at ph 10 EDTA FORMS 1:1 COMPLEX WITH BOTH Mg2+ and Ca2+ and after buffering at this pH a 10mL aliquot of the sample required 26.81mL of 0.003474M EDTA for titration The ...
Monday, March 12, 2012 at 4:43pm by jenny

chemistry
A stock solution of 0.0100 M KMnO4 is diluted by taking 15.5 mL of it and diluting it to 100.0 mL. From this diluted solution, 5.00 mL is taken out and diluted to 100.0 mL. What is the concentration of the solution obtained in the end
Tuesday, March 13, 2012 at 7:07pm by carla

chemistry
The urine excreted by an adult patient over 24 hours was collected and diluted to give 2.000L sample. at ph 10 EDTA FORMS 1:1 COMPLEX WITH BOTH Mg2+ and Ca2+ and after buffering at this pH a 10mL aliquot of the sample required 26.81mL of 0.003474M EDTA for titration The ...
Monday, March 12, 2012 at 5:19pm by TOM

Chem
pH = -log(H^+). Since the pH is a log function, the H^+ from 1 pH to the next (either higher or lower) is in steps of 10. That is pH = 2 is 10x weaker than a pH of 1 and 10x stronger than a pH of 3
Tuesday, May 4, 2010 at 8:26pm by DrBob222

Chemistry
A = pH of 8. 1,000 times means difference in pH of 3. If it is more H^+, then pH = 5 for the new solution. Is that acid or basic. pH<7 = acid pH=7 = neutral pH>7 = basic
Monday, November 14, 2011 at 3:56pm by DrBob222

science HElp
Ph scale Which on is true A substance with ph is twice as acidic as substance with ph of 4. A subtances with ph 3 is 10 as acidic as substance with ph of 4. A substance with ph 3 twice as alkies as substances with ph 4. a substancs with ph 3 10 time alkies as substance with ph...
Wednesday, November 23, 2011 at 7:14pm by shan

Chem
I don't get how to do this: What is the pH of the solution created by combining 11.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first...
Monday, October 29, 2007 at 4:00am by Anne

chemistry
A 500 ml bottle of 16 M hydrocholric acid is diluted to a final volume of 5,0 liters .. what is the concentration of the new diluted , HLC sloution
Wednesday, May 2, 2012 at 1:29pm by Anonymous

Chemistry
How many moles of NaOBr- must be mixed with 0.1788 mole of HOBr and diluted to 1L to prepare a solution having a pH of 8.7043. Ka of HOBr = 2.0 * 10-9
Saturday, April 16, 2011 at 1:11am by Jude

science
Are the following substances acid, base, or neutral: sodium bicarbonate (pH = 8.3): Blood (pH = 7.4): milk (pH =6.7): orange juice (pH = 3.6): milk of magnesia (pH = 10.5): How do you come up with the answers?
Monday, March 12, 2012 at 3:56pm by long

chemistry
which solution has the highest concentration of hydroxide ions? a ph=7.93 b ph=12.59 c ph=7.00 d ph=9.82 e ph=3.21 i know the answer is 7 but why is it seven? would it be different if it said hydronium ions?
Saturday, December 11, 2010 at 1:07pm by jessie

chemistry
Sr(OH)2 ==> Sr^+2 + 2OH^- pH = 13.12 pH + pOH = pKw = 14 and pOH = 0.88; therefore, (OH^-) = 0.132 What is the concn of the OH- in the satd soln? It is 0.132. That 15 mL is diluted to 250; now the concn is 0.132 x 15/250 = 0.00792M. We take 15 mL of that and titrate it with...
Monday, April 11, 2011 at 5:04am by DrBob222

chemistry
What is the pH of the solution created by combining 11.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? What are the pH values for HCl and HC2H302 if you take into account that the 8.00 mL of 0.10 M Acid was first diluted...
Friday, May 2, 2008 at 1:04am by Trisha

chemistry
A chemist dilutes 144.0 mL of 0.0743 M HCl with 775.0 mL of water. Determine the pH of the diluted solution. 1.86, 1.13, 2.08, 1.93, 12.07
Monday, December 5, 2011 at 2:39pm by Anonymous

Chemistry
thank Dr.Bob222 I see you got the same answer I did. I got one more I need help with if you can help me please Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 5:37pm by norma

Chemistry
How will the addition of sodium acetate to an acetic acid solution affect the pH? A. solution becomes hotter B. It will lower the pH C. It will raise the pH D. pH will not change E. pH cannot be measured I selected answer D and got it wrong. I don't understand why...
Sunday, March 10, 2013 at 12:18pm by Lisa

Chemistry
a. pH = -log(H^+) pH = -log(7E-4) pH = -(-3.15) pH = 3.15 b. pH + pOH = pKw = 14 pH + 6 = 14 pH = 8 The problems asks for (H^+); therefore, pH = -log(H^+) 8 = -log(H^+) -8 = log(H^+) (H^+) = 1E-8
Tuesday, April 30, 2013 at 11:21pm by DrBob222

Algebra
Is this correct? If not can you please tell me what steps I did wrong? Thanks! The hydrogen ion concentration of milk is about 1.6 x 10^-7 moles per liter. Find the pH. pH = -log [H+] pH = -log[1.6 x 10^-7] pH = -(-7.204119983) pH = 7.2 The pH balance of the milk is 7.2
Friday, June 18, 2010 at 8:41pm by Kate

Chemistry
2.87 for pH of 0.1M HAc is right. For HCl + HAc first, what is the concn of the HCl added? If we assume it is 0.1M (and it may not be that at all but you can adjust). (HAc) = 0.1M x (100/150) = 0.0667 (H^+) = x from HAc and 0.0333 from HCl (that is 50 mL x 0.1M diluted to 150 ...
Thursday, October 20, 2011 at 1:21pm by DrBob222

Chemistry
Hi,can I have your help? I'm just trying to solve a few Dilution Solution problems. I'm stuck on these two,and I wish you could help. Here's one: A 500 mL bottle of concentrated acetic acid is diluted to make a 5.0% solution. Find the volume of diluted that is prepared? ...
Wednesday, December 8, 2010 at 11:36am by Cliff

Chemistry
I am hoping to receive help getting started with this problem, possibly some steps in the correct direction. Here is the question: 5.0mLs of a 6.0M solution of HCl was transferred to a 1000ml volumetric flask and diluted to volume w/ water. 50mLs of this solution was then ...
Tuesday, June 9, 2009 at 6:31pm by Juggernaut

Chemistry
Then calculate the inital ClO^- concencentrations for 1st, 2nd, and 3rd reactions. Chemical reaction: Blue dye + ClO^- -->oxidized dye +Cl^- Reaction #1: 5.0 mL or diluted bleach solution, 15.0mL of distilled water, 10.0 mL of diluted blue dye Reaction #2: 10.0mL of diluted...
Monday, February 27, 2012 at 11:36pm by Cassandra

chemistry
1 ml of diluted solution is added to 9 ml of deionized water. predist the ph of resulting solution
Friday, July 30, 2010 at 3:35am by Anonymous

CHEMISTRY
calculate the ph of resulting solution when 2.50 ml of the 2.60 M acetic acid is diluted to make a 250.0 ml solution
Sunday, February 13, 2011 at 10:14pm by TYLER CHIRECE

CHEMISTRY
calculate the ph of resulting solution when 2.50 ml of the 2.60 M acetic acid is diluted to make a 250.0 ml solution
Sunday, February 13, 2011 at 10:15pm by TYLER CHIRECE

Chemistry
How many millimeters of this solution should be diluted with water to produce 650 mL of a solution with pH= 11.50? 6.8% ammonia (d= 0.97g/ml)
Saturday, February 14, 2009 at 4:44pm by Raj

Chemistry
Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037 formic acid (HCOOH; pKa = 3.75) solution (diluted to 100 mL volume with deionized water) by 0.0964 M solution of KOH. I have to determine volume of KOH needed to reach equivalence point, the pH of ...
Monday, March 5, 2012 at 6:10pm by Clint

Chemistry DrBob
its two sorry the whole thing that i wrote didn't show up again. What is the pH of the solution created by combining 2.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)? Here is the chart that i am supposed fill out: mL ...
Thursday, May 1, 2008 at 4:53pm by Amy

AP Chemistry
A buffer solution contains .4mol of formic acid, HCOOH and a .6mol of sodium formate, HCOONa, in 1L of solution. Ka of formic acid is 1.8 x 10^-4. a) calculate pH b) if 100ml of this buffer solution is diluted to a volume of 1L with pure water, the pH does not change. Discuss ...
Sunday, April 25, 2010 at 12:24pm by Jessie

chemistry
pH pure H2O = 7 (H^+) = (OH^-) = 1E-7M acid pH < 7 base pH > 7 neutral pH = 7
Sunday, April 21, 2013 at 12:44pm by DrBob222

chemistry
No, that isn't correct. The more acidic the solution, the lower the pH. pH <7 = acid pH = 7 neutral pH >7 = basic
Tuesday, November 8, 2011 at 6:27am by DrBob222

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks
Thursday, May 5, 2011 at 12:38pm by Renee

Chem
A particular household ammonia solution ( d= 0.97 ) is 6.8% NH3 by mass How many milliliters of this solution should be diluted with water to produce 600 ml of a solution pH= 11.65?
Monday, February 16, 2009 at 6:48pm by Kyle

chemistry
.70 L of a buffer solution that is 0.120 M in NH3 and 0.450 M in NH4Cl are diluted to 5.80 L with distilled water. What is the pH of the buffer? Kb of NH3 = 1.8 x 10^-5
Friday, October 8, 2010 at 10:30pm by kim

chemistry
30.0 mL of 1.50 M NaOH is diluted to 50.0 mL. What is the resulting pH?
Monday, February 28, 2011 at 3:58pm by Anonymous

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