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April 20, 2014

# Search: what is the pH of a solution that is made by combining 125 {\rm mL} of .04 M hydrofluoric acid with 50.0 {\rm mL} of 0.11 M sodium fluoride

Number of results: 6,779

Chem
What stoichiometric concentration of the indicated substance is required to obtain an aqueous solution with the pH value shown below? a)aniline, C6H5NH2, for pH= 9.05 b)NH4Cl for pH= 5.22
Friday, March 2, 2012 at 8:41pm by Ashley

Chemistry
Any numbers; however, I suspect you are asking which pH values show acid and which show base. pH = 7 is neutral. pH<7 = acid pH>7 = base.
Tuesday, May 4, 2010 at 7:48pm by DrBob222

Chem
Perhaps you have misread the question. For the first one, (H3O^+) = 1.5E-8 pH = -log(H^+) pH = -log(1.5E-8) pH = -(-7.82) pH = 7.82.
Wednesday, December 1, 2010 at 3:33pm by DrBob222

Chemistry
I'm not sure what you mean. Do you mean pH of 1/2 or pH at the 1/2 way point. pH = 0.5 gives (H^+) = 0.316 M. pH at the 1/2 way point is pKa whatever that is (depends upon the acid).
Thursday, April 26, 2012 at 11:43am by DrBob222

Chemistry
Do you know the definition of pH? pH = -log(H^+) For HCl, which is a strong acid (a strong electrolyte meaning it ionizes 100%), (H^+) is same as (HCl). Therefore, pH = -log(0.1) Punch 0.1 into your computer, hit log and you will get -1. So pH = -(-1) = +1. OK?
Thursday, October 1, 2009 at 1:33pm by DrBob222

chemistry
How to calculate PH 1.9 = 0.0126M Why? How to calculate PH 1.8 = ? How to calculate PH 20 = ? How to calculate PH 21 = ? Pls helps me
Sunday, August 5, 2012 at 1:09pm by Fai

chemistry
In a buffer solution, if [Aƒ{] < [HA], which of the following must be true? a. pH < pKa b. pH = pKa c. pH > pKa d. pH < 7.00 e. pH > 7.00
Wednesday, November 10, 2010 at 4:13pm by miller

chemistry
No. Isn't the first column mL NaOH and the second column is pH. Then between pH 6.5 and 11.2 or so is the vertical portion of the pH and that occurs about 12 mL or so if I read your numbers correctly. A pH of 12 is at 15.0 mL and the curve in that region is almost horizontal.
Saturday, April 5, 2008 at 5:22pm by DBob222

Chemistry
Im not sure how to edit and it didnt line up right, so Im just going to write it out. I have to figure the following from the one answer. (H+1) M, pH, (OH-1)M, pOH H+1 = 2.5x10^-5 = need pH, OH-1 and pOH pH = 2.5 --> need H+1, OH-1 and pOH OH-1 = 5.2x10^-2 --> need, H+1...
Monday, April 1, 2013 at 8:20pm by Kishwa

Chemistry
Use the Henderson-Hasselbalch equation. For A. pH = pKa + log (base)/(acid) pH = pKa + log(ClO^-)/(HClO) pH = pKa + log(0.09)/(0.09) pH = pKa + log 1 pH = pKa.
Monday, March 4, 2013 at 8:53pm by DrBob222

Chemistry
I got initial PH= 9.24 PH after HCl addition= 9.19 PH after NaOH addition= 9.3 so delta PH after HCl= 0.05 delta PH after NaOH= - 0.06 all these still wrong answers. could it be that I'm calculating the total volume wrong? should be 0.01+0.006 L?
Tuesday, March 27, 2012 at 6:01pm by Mima

Chem
a. mols NaOH = grams/molar mass = 26.9/40 = about 0.67 and that divided by 0.5 = about 1.35M pH = -log 1.35 pH = -(0.13) = -0.13 approximately. Remember 1.0M = zero pH. b. And it is that simple. It's that negative pH again. HI = 1.62M (H^+) = 1.62M pH = -log(1.62) = about -0....
Wednesday, February 27, 2013 at 9:02pm by DrBo222

Chemistry 130
[H+}=10^-5 pH=5 [H+]=10^-2 pH=2 Thus: The greater the hydrogen concentration the lower the pH. So is this direct or inverse relationship?
Tuesday, October 13, 2009 at 10:53am by Dr Russ

chemistry
Very good. That's the first step. Now step 2 is even easier. pH + pOH = pKw. pH + 9.21 = 14. pH = ??
Wednesday, May 7, 2008 at 9:32pm by DrBob222

ap chem
Convert pH 3.0 to (H^+) using pH = -log(H^+). Convert pH 5.6 to (H^+). Divide 1st by the 2nd to find the ratio acid/normal
Monday, February 14, 2011 at 12:21am by DrBob222

chemistry
just use the formula pH + pOH = 14.0 where pH is unknown and pOH is currently the pH given in the question because, it is a weak base.
Friday, May 31, 2013 at 1:36am by barco

chem class
What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion? i posted this before and i tried solving it but i get it wrong 14 = ph + - log (3.98 × 10-9) 14- 8.4 = ph 5.6 = ph but the correct answer is 8.400 what did i do wrong?
Sunday, November 21, 2010 at 7:51pm by jessie

Chemistry
Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B: [H+]=?[OH-]=1.4e-6M pH=? pOH=? Solution C: [H+]=?[OH-]=? pH=5.36 pOH=? Solution D: [H+]=?[OH-]=? pH=? pOH=10.14
Thursday, October 20, 2011 at 10:08pm by Help

Chemistry
Complete this table of values for four aqueous solutions at 25 °C. Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B: [H+]=?[OH-]=1.4e-6M pH=? pOH=? Solution C: [H+]=?[OH-]=? pH=5.36 pOH=? Solution D: [H+]=?[OH-]=? pH=? pOH=10.14
Thursday, October 20, 2011 at 11:30pm by Help

chem
I have to find the effective pH range of a buffer. I read that this optimal buffering occurs when the pH is within 1 pH unit from the pK value for the buffering system. But can anyone explain why its is optimal within 1 pH unit? Thanks.
Saturday, January 28, 2012 at 9:34pm by ian

chemistry
after finding the ph of the corresponding ions in these two questions, would you add the two ph's together to determine the final ph of the solution?
Saturday, April 18, 2009 at 3:05pm by Anonymous

Chemistry
pH 13.95; convert to H^+ by pH = -log(H^+) and change to OH. Then convert pH 9.066 to OH^- the same way. mLsoln1 x Msoln1 = mLsoln2 x Msoln2.
Tuesday, January 17, 2012 at 2:19pm by DrBob222

biochemistry
pH=7.20+log 0.2M/ 0.4M pH=7.20+(-0.30) pH=6.69 I'm heading in the right direction?
Friday, January 21, 2011 at 7:32pm by dIrk

emily
some skin creams claim that they are "pH balanced" and yet do not have a pH of 7. what do they mean when they say pH balanced?

Chemistry - pH
This has a very good explaination. Go thru his examples, especially at the end. On c, find the OH concentration, then the pOH, then you know pH+pOH=14 and you can solve for pH from that.
Monday, September 14, 2009 at 10:12am by bobpursley

Chemistry
The pH of a solution is 11.30. In order to find the concentration of H+, wouldn't I simply take the pH of the solution and plug it into the formula 10^-pH?
Wednesday, September 16, 2009 at 11:21pm by Anonymous

Chemistry
The number in the pH is equal to the negative exponent of 10. So, a pH of 7 has a concentration where the exponent is -7, a pH of 9 will have an exponent equal to -9 and so on. So the lowest pH will have the highest H ion concentration. 10^-3 is bigger then 10^-9. So the ...
Tuesday, March 19, 2013 at 7:26pm by Devron

chemistry
What should be the pH of the aqueous layer to extract caffeine? There are three aqueous solutions that you may choose from. Answer A. pH >14, using 2.5 M NaOH (aq) B. pH 1, using 0.1 M HCl (aq) C. pH 6.2, using 0.1 M NaHCO3 (aq)
Thursday, May 30, 2013 at 9:41am by A

chemistry
What should be the pH of the aqueous layer to extract caffeine? There are three aqueous solutions that you may choose from. Answer A. pH >14, using 2.5 M NaOH (aq) B. pH 1, using 0.1 M HCl (aq) C. pH 6.2, using 0.1 M NaHCO3 (aq)
Thursday, May 30, 2013 at 6:04pm by A

chemistry
Na2CO3. The CO3^-2 ion hydrolyzes as follows: CO3^-2 + HOH ==> HCO3^- + OH^- Thus you see OH^- is produced; the pH should be basic. By the way, it is pH and not Ph.
Tuesday, March 15, 2011 at 11:51pm by DrBob222

CHemistry
you want to measure the rate of change of pH? Not knowing what you are doing, the simple answer is to put a pH indicator in the solution and proceed with the change process, monitoring pH vs time.
Wednesday, November 2, 2011 at 9:59am by bobpursley

Chemistry
Calculate the pH of a solution in which a. [H3O+] = 7.8 x 10-7 M pH = b. [H3O+] = 5.1 x 10-6 M pH = c. [H3O+] = 6.1 x 10-5 M pH = d. [H3O+] = 9.3 x 10-4 M pH = I get 8.1 9.5 9.1 6.7 but its wrong please someone help!
Wednesday, March 19, 2014 at 5:03pm by Danny

university chemistry
this is for a chemistry laboratory experiment called "how much caffeine is there in instant coffee" What should be the pH of the aqueous layer to extract caffeine? There are three aqueous solutions that you may choose from. A. pH >14, using 2.5 M NaOH (aq) B. pH 1, using 0....
Tuesday, March 12, 2013 at 9:11am by angela

Chemistry
I don't readily see anything wrong with the answer by anonymous; however, it's a lot of unnecessary work. You don't need to go through the OH or pOH. pH = -log(H^+) pH = -log(0.1) solve. pH = 1
Wednesday, September 30, 2009 at 7:04pm by DrBob222

Chemistry
A buffer solution of volume 100.0 mL is 0.150 M Na2HPO4(aq) and 0.100 M KH2PO4(aq). Refer to table 1. (a) What are the pH and the pH change resulting from the addition of 80.0 mL of 0.0500 M NaOH(aq) to the buffer solution? pH pH change (include negative sign if appropriate) (...
Tuesday, March 16, 2010 at 11:52pm by Trixie

CHEMISTRY
You subtract the moles of NaoH from the moles of HCl to determine the excess moles left, which decides the pH. To find pH, pH= -log(concent. of H+) or ( concen. of OH-) If NaOH is more than HCl, you get find pH by subtracting the pOH you get from the above formula from 14.
Sunday, October 17, 2010 at 4:50pm by Rose

Chemistry
How can I suggest a reason for the deviation for the pH of 4 M HCl? As my answer I put, The pH of 4 M HCl is negative because a molarity of an acid solution greater than 1 produces a negative pH. A negative pH means that the concentration of H+ or H3O+ ions is greater than 1 ...
Wednesday, March 7, 2007 at 12:18pm by Meche

Chemistry
pH = -log(H^+) and pH + pOH = pKw = 14. lime juice pH will give you H^+ (technically it is H3O^+) If you know pOH, you can solve the other equation to obtain pH. Also you can use pOH = -log(H^+) OR you can use (H^+)(OH^-) = Kw = 1E-14.
Wednesday, April 4, 2012 at 10:33pm by DrBob222

chem
hey guys I posted this awhile ago im not sure if anyone has read it or whatever but here it is again find the PH of a .00580 M solution of the strong base KOH. is it -log(.00580)= 2.24 pOH = -log[OH-] pH + pOH = 14.00 Therefore, pOH = -log(.00580) pH + 2.24 = 14 pH = 11.76 ...
Thursday, March 22, 2007 at 11:09pm by chris

Chemistry
• Describe the properties of acids and bases and explain the concept of pH • How will you measure the pH of the soil in your garden • How will pH affect materials and equipment you might use in gardening. • 3 vegetables and 3 flowers that would work well together in a small ...
Sunday, March 24, 2013 at 3:47am by Juan

chemistry
I didn't get an answer since the log of a negative number is not possible. The problem would work if it was 100 mL of 0.1 M (instead of the 50 mL). Then we would have B = 0.00334 - 0.002 A = 0.00667 + 0.002 pH = 8.3 + log 0.00134/0.00867 pH = 8.3 + log 0.155 pH = 8.3 -0.811 pH...
Monday, February 4, 2008 at 8:54pm by drbob222

chem
pH = -log(H^+). Substitute and solve for pH. Then pH + pOH = 14 to obtain the pOH.
Wednesday, April 28, 2010 at 11:02pm by DrBob222

College Algebra
The hydrogen ion concentration of a substance is related to its acidity and basicity. Because hydrogen ion concentrations vary over a very wide range, logarithms are used to create a compressed pH scale, which is defined by pH=-log(H+)where (H+)is the hydrogen ion ...
Monday, December 8, 2008 at 1:54am by Jenny

Chemistry (or Physio/Biochem)
Asthma affects about seven percent of the population. During an asthma attack smooth muscle cells in the bronchi constrict, the airways become inflamed and swollen, and breathing becomes difficult. What effect might an asthma attack have on blood pH? A. pH goes down B. pH goes...
Sunday, March 14, 2010 at 9:14pm by Trixie

science
Assume that you have a pH meter which would enable you to very accurately measure the pH of a solution. Describe an experimental design that would allow you to pinpoint the exact pH at which Catalase is the most active.
Friday, March 11, 2011 at 9:35am by anonymous

Chemistry
Assuming equal concentrations , rank these solutions by pH. RbOH(aq), NH3(aq), HF(aq) HBr(aq), Ca(OH)2(aq). I know the most acidic solution has the lowest pH and the most basic solution has the highest pH. But how am i supposed to know the pH if i don't know the concentration ...
Monday, October 17, 2011 at 11:12pm by Nia

STATS
Samples of both surface soil and subsoil were taken from eight randomly selected farms in a county. The soil samples were analyzed to determine both surface pH and subsoil pH, which yielded the following results: Farm 1 2 3 4 Surface pH: 6.55 5.98 5.59 6.17 Subsoil pH: 6.78 6....
Tuesday, February 22, 2011 at 6:02pm by Rina

science
What is the [Pb+2] in a saturated solution of Pb(OH)2 for each of the following initial pH values? Ksp Pb(OH)2 = 2.8x10-16 a. pH = 13.00 b. pH = 9.20
Monday, January 31, 2011 at 11:48am by N/A

AP CHEMISTRY
a and b are salts. The pH of those solutions is determined by the hydrolysis of the salt. c is a mixture; you calculate the molarity of the acetate ion and go from there. Here is how you do the first one, in detail. .............F + HOH ==> HF + OH^- initial.....0.1...
Thursday, February 16, 2012 at 4:36pm by DrBob222

Chemistry
For the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaoH, calculate (a) the initial pH; (b) the pH when neutralization is 50% complete; (c) the pH when neutralization is 100% complete; and (d) the pH when 1.00 mL of NaOH is added beyond the equivalence point.
Tuesday, August 11, 2009 at 7:25am by ChemHurts

Chemistry
Which of the following is correct? A)A substance with pH of 3 is 10 times as Acidic as a substance with a pH of 4. B)A substance with a pH 3 is twice as acidic as a substance with a pH of 4.
Thursday, April 12, 2012 at 11:21am by Lee

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
Frankly I don't know what it's asking unless by titration they mean the HCl has been exactly neutralized. If that is the case, then the pH will be 7.0 because the salt produced is NaCl and neither the cation nor the anion is hydrolyzed. The other interpretation is that the ...
Wednesday, March 21, 2012 at 7:34pm by DrBob222

chemistry
Now take another 35 mL of the 0.50 M pH 6.59 buffer and add 1.5 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution. find pH
Monday, October 24, 2011 at 2:53pm by Taylor

science
calculate the pH of pure water. (recall that pH= -log[H+]) Hopefully the following site will help you: http://en.wikipedia.org/wiki/PH
Saturday, December 30, 2006 at 10:11pm by michelle

Math
H+(conc) = 10^-pH So, in the first case, H+ = 10^-4 in the second case, the concentration of H+ = 10^-8 Subtract these two to find the difference, or divide the two to find a ratio expressing the change. A pH below 7 is acidic, a pH above 7 is basic, so increasing pH means the...
Wednesday, October 17, 2012 at 9:46am by Jennifer

Chemistry
The pH of healthy lakes is around 6.0. Due to acid rain, the pH of our lakes & rivers is decreasing. At low pH levels, producers such as phytoplankton cannot thrive. Decreased plankton can cause consumer populations to crash. The end result is a lake devoid of life. If the pH ...
Sunday, December 16, 2007 at 12:12am by Lucy

science
Can you tell me on the pH scale what no.s are acid and what are alkali please. I have found some info but have not yet learnt pH scale. My pH scale goes from 0 (hydrochloric acid) to 12 (ammonia). Thanks http://en.wikipedia.org/wiki/PH
Sunday, November 5, 2006 at 1:50pm by red again

Honor Biology
Remember that the greater the concentration of hydrogen ions, the lower the pH of a solution. How do you suppose the pH of the solution in the thylakoid space compares with the pH of the solution in the stroma? What is responsible for the difference?
Monday, December 6, 2010 at 4:02pm by Pam

Chemistry
Posted by Hannah on Saturday, April 18, 2009 at 3:05pm. Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2. Responses * chemistry - Anonymous, Saturday, April 18, 2009 at 3:36pm after finding the ph of the corresponding ions in these two ...
Saturday, April 18, 2009 at 3:43pm by Anonymous

Chemistry
what is the pH of Sulphuric acid? It depends upon the molarity. pH = -log(H+) -log = ? pH = -log(H^+) find (H^+), punch that into your calculator, change the sign to minus, then find the "log" key and punch that. That will be the pH.
Monday, March 12, 2007 at 5:17pm by Gemma

Chemistry
An amino acid has the form shown at R-CH-C-O^- (with a NH2 bonded to the CH and a O double bonded to the C) (O^- means the C has a negative charge) a) a pH of 7.0 b) any pH other than 7.0 c) a pH greater than its isoelectric point d) its isoelectric point e) a pH less than its...
Thursday, March 25, 2010 at 8:13pm by Holly

chemistry lab
Hi, so I did a lab on acids, bases, salts and buffer solutions. After measuring the pH for a .010 M HCl solution I got a pH of 2.50. After doing a calculated pH of .010 M of HCl the answers is 2. My question is why do you think my pH from the experimental is slightly higher ...
Tuesday, March 27, 2012 at 9:57pm by maura

Honors Biology - URGENT!!!
Remember that the greater the concentration of hydrogen ions, the lower the pH of a solution. How do you suppose the pH of the solution in the thylakoid space compares with the pH of the solution in the stroma? What is responsible for the difference?
Wednesday, December 8, 2010 at 8:15am by Brenda

Chemistry
I figured out the correct new pH for each respective part, but apparently the initial pH i found for the buffer solution is incorrect. I just need help in figuring that so I can calculate the change. I initially thought the buffer pH was 7.38. Thanks!
Tuesday, March 16, 2010 at 11:52pm by Trixie

Chemistry
1. Chemists define pH as "the negative logarithm of the concentration of protons". In mathematical terms: pH = - log [H+] What is the pH of a solution whose [H+] is 0.0007 M? i got it as 7.0 i know it is wrong 2. What is the [H+] in a solution having a pOH of 6 ? isn't it ...
Tuesday, April 30, 2013 at 11:21pm by Lynn

Chemistry
pH = 5 pH + pOH = pKw = 14 from which you can find pOH. Then pH = -log(H^+) and pOH = -log(OH^-). If pH = 5, then H^+ = 1E-5. You get that straight from the calculator. If pH = 5, then pOH = 9 and OH^- = 1E-9 (straight from the calculator) but you can do those in your head.
Wednesday, May 25, 2011 at 10:09pm by DrBob222

Chemistry
An amino acid will have the form shown at: R-CH-C-OH (with an O double bonded to the C and a NH3+ bonded to the CH) a) a pH of 7.0 b) any pH other than 7.0 c) a pH greater than its isoelectric point d) its isoelectric point e) a pH less than its isoelectric point Would it be "...
Thursday, March 25, 2010 at 8:16pm by Holly

chemistry
a. neither Na^+ nor Cl^- are hydrolyzed; therefore, the pH is just that of pure H2O which is pH = 7. b. KCN the CN^- is hydrolyzed. CN^- + HOH ==> HCN + OH^- so you know it will be basic. You can calculate the actual pH but that isn't necessary. c. LiF the F^- is hydrolyzed...
Tuesday, March 26, 2013 at 11:04pm by DrBob222

Chemistry
10.00 mL of an unknown base solution is titrated with .100 M HCl solution. The pH versus the volume of NaOH added is shown below. There is a graoh where there are two dotted lines signifying a pH: the highest at pH 6.31 and the lower at pH 3.92. What is the pOH pf the solution...
Thursday, March 27, 2014 at 5:58pm by Dezzi

CHEMISTRY--URGENT
HNO3 with pH 3 is mixed with 2 L KOH with pH 12. assuming volumes are additive what is the pH of the final solution? I have absolutely no idea how to do this. I do know the answer, though. I have a test tomorrow and I would really appreciate it if someone could help!!!!
Sunday, May 2, 2010 at 11:59pm by Maggie

Pre Calculs
The pH of a chemical solution is given by the formula pH = -log10 [H+] where [H+] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). (a) what is the pH of the solution for which [H+] is 0.1? (b) What happens to pH as ...
Tuesday, October 10, 2006 at 1:06pm by Erica

chemistry class
What is the pH of an aqueous solution at 25.0 °C that contains 3.98 × 10-9 M hydroxide ion? i posted this before and i tried solving it but i get it wrong 14 = ph + - log (3.98 × 10-9) 14- 8.4 = ph 5.6 = ph but the correct answer is 8.400 what did i do wrong? or is the answer ...
Monday, November 22, 2010 at 9:31pm by jessie

Ph CHEM
pOH = 4 pH = 10 Or (H^+) = 1E-14/1E-4 = 1E-10 pH = 10 The data base is wrong or you posted the problem incorrectly. The pH is 10 for the above problem.
Tuesday, November 27, 2012 at 9:31pm by DrBob222

pH
what's the pH of the acid HCl with concentration of .15? the acid HC2H3O2 with concentration of .15? I figured out the pH of HCl, but I'm still not sure how to find the other one... What is the dissociation constant for acetic acid? K= [H+][ace-]/.15 pH= -log sqrt (.15 k) ...
Saturday, April 14, 2007 at 6:25pm by Christine

chemistry
Consider the titration of 21.0 mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. what is the initial pH? what is the volume of added base required to reach equivalance point? what is the pH at 5.00 mL of added base? pH at one half o the equivalence point? pH at the equivalence ...
Thursday, July 29, 2010 at 4:23pm by Ellen

Chemistry
Rank these to highest pH to lowest pH: NH3, KOH, Ca(OH)2, HBr, HBrO I put these in the same order for highest pH to lowest but still get it wrong.
Wednesday, February 20, 2013 at 10:52pm by Anon

Chemistry
DrBob22 please help with the pH. I am not sure if I would use pKa=-logKa=-log(1.9*^-5)=4.74 or do I use [H3O]= 10^-pH =.0040=10*^-ph
Sunday, March 25, 2012 at 12:30pm by Mary

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
THe highest pH is the most basic. 14-pOH=pH pOH=-log[OH-] pH=-log[H+] Use the formulas and see if you are correct, but I believe that you are.
Tuesday, February 12, 2013 at 8:56am by Devron

chemistry
a) Aluminum Chloride has a universal indicator color of red and the Ph of 4.0 b) Sodium Carbonate has a universal indicator color of violet and the Ph of 9.5. c) Ammonium Acetate has a universal indicator color of green and the Ph of 7.5 For the following salts give an ...
Tuesday, March 15, 2011 at 2:20pm by samuel

chemistry
) Aluminum Chloride has a universal indicator color of red and the Ph of 4.0 b) Sodium Carbonate has a universal indicator color of violet and the Ph of 9.5. c) Ammonium Acetate has a universal indicator color of green and the Ph of 7.5 For the following salts give an ...
Tuesday, March 15, 2011 at 4:27pm by roshan

chemistry
Aluminum Chloride has a universal indicator color of red and the Ph of 4.0 b) Sodium Carbonate has a universal indicator color of violet and the Ph of 9.5. c) Ammonium Acetate has a universal indicator color of green and the Ph of 7.5 For the following salts give an ...
Tuesday, March 15, 2011 at 10:44pm by roshan

Chemistry
Hi I'm doing a research paper on the PH of skin and was wondering if you could answer even a few of these questions. I am in high school. Thanks. what does ph have to do with skin? how would using alkaline products affect skin? what are some symptoms caused by using the wrong ...
Tuesday, May 6, 2008 at 11:12pm by Anonymous

chemistry
pH = -log(H3O^+) pH = -log(5.5E-3) pH = -(-2.26) pH = +2.26
Monday, April 29, 2013 at 10:02pm by DrBob222

ap chemistry
for the following, mix the equal volumes of one solution from group I with one solution from group II to achieve the indicated pH. calculate the pH of each solution. Group I: .2M NH4Cl, .2M HCl, .2M C6H5NH3Cl, .2M (C2H5)3NHCl Group II: .2M KOI, .2M NaCN, .2M KOCl, .2M NaNO2 a...
Thursday, February 9, 2012 at 12:17am by hannah

chemistry 2
Titration of 50.0 mL of acetic acid reaches equivalence after delivery of 22.5mL of standardized NaOH 0.21 M. What is the initial concentration of acetic acid and what is the pH of the solution? What is the pH at equivalence? What is the pH adition of 20.0 mL of NaOH? What ...
Monday, April 14, 2014 at 2:31pm by philip

Chemistry
1) A solution that is made out of 1.00mol/L ammonia and 0.50mol/L of ammonium chloride is a basic buffer. pH = pKa + log(base/acid) pH = 9.25 + log(1.00/0.5) pH = 9.55 basic.
Saturday, December 8, 2012 at 2:54pm by DrBob222

Chemistry
Calculate the amount of H2SO4 needed to make 1.00L of acid rain with a PH equal to the average PH of rain in Maine (ph = 5.0). Concentration of H2SO4 to use = .00100M I am absolutely confused...please help
Wednesday, January 23, 2013 at 6:24pm by Henry

chemistry
Aluminum Chloride has a universal indicator color of red and the Ph of 4.0 b) Sodium Carbonate has a universal indicator color of violet and the Ph of 9.5. c) Ammonium Acetate has a universal indicator color of green and the Ph of 7.5 ....For the following salts AlCl3, Na2CO3...
Tuesday, March 15, 2011 at 10:44pm by roshan

chemistry
Aluminum Chloride has a universal indicator color of red and the Ph of 4.0 b) Sodium Carbonate has a universal indicator color of violet and the Ph of 9.5. c) Ammonium Acetate has a universal indicator color of green and the Ph of 7.5 ....For the following salts AlCl3, Na2CO3...
Tuesday, March 15, 2011 at 11:51pm by roshan

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
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
A potassium hydroxide solution has a pH of 12.90. Enough cid is added to react with half of the OH- ions present. What is the pH of the resulting solution? Assume that the products of the neutralization have no effect on pH and that the amount of additional water produced is ...
Tuesday, May 4, 2010 at 7:37pm by Alexa

Chemistry
pH = -log(H^+) Plug in 6 for pH and calculate (H^+). Then remember that pH + pOH = 14 and do OH^- the same way (except plug in 8 for pOH).
Tuesday, August 28, 2007 at 9:22pm by DrBob222

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
The Henderson-Hasselbalch equation is pH = pKa + log [(base)/(acid)] pKa = 4.74 from Ka. Generally it is easy to prepare a buffer within 1 pH of the pKa. You can work through the calculation if you wish; for example, if equal amounts of acid and base are chosen, then (B) = (A...
Wednesday, August 6, 2008 at 12:18am by DrBob222

chemistry
1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution? 2) A 0.25 M solution of a monoprotic acid, HA, has a pH of 2.54. What is Ka for this acid? The dissociation of HA is: HA + H2O <--> H3O+ + A- (Hint: write the expression for pH) 3 A solution has...
Sunday, December 9, 2012 at 3:17am by nicki

chemistry
Given pH = 4.67, pH = ? pH = -log(H^+) 4.67 = -log(H^+) -4.67 = log(H^+) (H^+) = 2.29E-5 Here is how you do it on the calculator. Punch in 4.67. Hit the change sign to it becomes -. (If you don't have a change sign, punch in -4.67 at the start.) Now locate and hit the 10x key...
Friday, November 11, 2011 at 8:40am by DrBob222

Chemistry
If you know H^+ or OH^- the other can be calculated from (H^+)(OH^-) = Kw = 1E-14 If you want pH pH = -log(H^+) If you want pOH pOH = -log(OH^-) If yo have pH or pOH and want the other one pH + pOH = pKw = 14
Tuesday, March 11, 2014 at 7:30pm by DrBob222

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