Search: calculate pH HClO2

Number of results: 25,067

chemistry
A swimming-pool worker wants the pool's pH to be 7.2. She comes by to test the water and finds that the pH is 9.2. What should she do to correct this situation?
Friday, March 9, 2012 at 2:32pm by princess

CHEMISTRY
Why does thymol blue change color at the pH that is does? I know it goes through transition one and transition two but I don't know why it changes at the pH that it does.
Saturday, February 25, 2012 at 7:05pm by TED

Biochemisty
If I take 5mL of a TRIS/HCL buffer with a pH of 7.4 and add 1mL of 1M HCL, how do I determine the new pH?
Wednesday, January 12, 2011 at 8:05pm by Rose

Chemistry
All you have to do is find the concentration of OH- and solve for pH (pOH= -log [OH-] nad then 14-pOH=ph [OH-} = Ksp/[M+}
Friday, March 19, 2010 at 8:16pm by Trixie

Chemistry
A buffer containing 0.2832 M of acid, HA, and 0.1504 M of its conjugate base, A−, has a pH of 2.36. What is the pH after 0.0015 mol NaOH is added to 0.5000 L of this solution?
Friday, March 16, 2012 at 1:29pm by Tracey

Chemistry
The approximate pKa values for the three dissociating groups of lysince are 2.2, 9.0, 10.5. What would the pH after addition of 10ml of 1.0M NaOH to 100ml of 0.1M lysine at pH 2.2?
Sunday, August 14, 2011 at 4:33pm by Mabel

Chemistry
Consider 57.5 mL of a solution of weak acid HA (Ka = 1.00 10-6), which has a pH of 3.800. What volume of water must be added to make the pH = 6.000?
Sunday, February 15, 2009 at 11:54pm by Brian

Sci
Where. pH levels in drinking water, in our bodies, in out soil, in outer space????? Remember that the "thing" which you are asking about will be more basic (less acid) if the pH increases.
Tuesday, September 2, 2008 at 11:20pm by DrBob222

Chemistry! Please Help!
Let's call propionic acid HP, then it will ionize as HP ==> H^+ + P^- First convert pH = 2.50 to (H^+) by pH = -log(H^+). Then set up the expression for Ka. Ka = (H^+)(P^-)/(HP). You know (H^+) now from the pH calculation. You know (P^-) because it equals the same ...
Thursday, February 12, 2009 at 7:46pm by DrBob222

chemistry
First what do we have? 100 mL x 0.1M NH3 = 10 millimoles. 100 mL x 0.1M NH4Cl = 10 mmoles. 6.00 mL x 0.1M HCl = 0.6 mmol. 6.00 mL x 0.1M NaOH = 0.6 mmol. I'll do one to show you how to do it. .........NH3 + H^+ ==> NH4^+ initial..10.....0.......10 add............0.6...
Saturday, February 4, 2012 at 2:12pm by DrBob222

chemistry
The pH at the beginning of the titration is just the pH of a 0.2 M HF solution. b). moles HF = M x L = ?? moles NaOH = M x L = ?? Which is in excess. Subtract. If HF in in excess, you will have a buffer solution of HF and NaF. If NaOH is in excess the pH will be determined by ...
Saturday, November 6, 2010 at 5:04pm by DrBob222

CHEMISTRY
pH = -log (H^+) 4.6 = -log(H^+) -4.6 = log(H^+) Take antilog both side. To do that on your calculator, key in 4.6, change to - 4.6, then hit the 10x key. That will give you 2.51 x 10^-5. For #2, convert pH 8.0 to pOH by remembering that pH + pOH = 14. Then pOH = -log(OH^-).
Thursday, June 3, 2010 at 8:56pm by DrBob222

Chemistry-pH
If you are given a colored substance as a sample, how would you measure the pH of a sample?
Tuesday, January 25, 2011 at 5:12am by Bam

Chemistry
yes, yes, and no. Yes it is 0.1 over 0.1, and yes log 1 = 0, but no, pH isn't 6.4 x 10^-5. pH IS, however, pKa since log 1 = 0.
Wednesday, May 5, 2010 at 8:14pm by DrBob222

Chem Titration and pH
Calculate the pH at 0mL, 5mL,...40mL for a 10.0mL aliquote of 0.100M Na3AsO4 (weak base) titrated with 0.100M HCl pKa1 = 2.25 pKa2 = 6.77 pKa3 = 11.60 Thank you First you should write equations to know where we are in the titration. At the beginning, we have the hydrolysis of ...
Saturday, October 7, 2006 at 6:15pm by julie

Chemistry
A 11.8 mL sample of a HCl solution has a pH of 2.000. What volume of water must be added to change the pH to 4.000?
Wednesday, November 23, 2011 at 7:07pm by Kaleen

Chemistry
pH = -log(concentration) pH of HClO4= -log(5.8x 10^-2 M) use a calculator and figure it out do the same for the second.
Sunday, March 21, 2010 at 8:08pm by Mohamed

chem
your first assumption was correct. you have to find the pH fo the final solution. the final pH will be one of the 5 options provided.
Saturday, March 7, 2009 at 11:34pm by Anonymous

science
What effect would a change in pH have on the effectiveness on catalase? But first of all, what is the ideal pH range for catalase activity?
Monday, September 10, 2007 at 9:31pm by Anonymous

Chemistry
I went ahead and did the calculations for you. I find that x is 0.001331654593 or x is -0.001331654593. I read your previous post and since you are looking for a concentration of ions, only the positive value matters. So you have 0,133 x 10^-2 mol/l H+ ions. If you want to ...
Saturday, January 19, 2008 at 5:50am by Christiaan

chemistry
Convert 14 g to moles. moles = grams/molar mass. M Ca(OH)2 = moles/L soln. (OH^-) = twice that of Ca(OH)2. Then pOH = -log(OH^-) and convert pOH to pH by pH + pOH = pKw = 14. Solve for pH.
Tuesday, December 13, 2011 at 10:33am by DrBob222

Pre-Algebra
Find each product or Quotient. Express using exponents. 1. The quotient of a to the 8th power and a to the 8th power? a 2. The quotient of -x to the 5th power and -x? -x to the 4th power 3. (15/5)(n to the 9th power/ n)? 3n go the 10th power Neutral water has a pH of 7. Each ...
Tuesday, January 18, 2011 at 9:07pm by TiffanyJ

Chemistry
What is the pH of the solution created by combining 11.40 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 NaOH pH w/ HCl pH w/ HC2H3O2 11.40 _________ ____________ Here'...
Monday, April 27, 2009 at 7:32pm by Lisa

Chemistry - pH
a) 0.35M HCl (monoprotic strong acid) produces a 0.35M [H+] solution. pH = -log(0.35) c) 0.35M NaOH (strong base) acid produces a 0.35M [OH-] solution. pOH = -log(0.35) pH = 14-pOH b) 0.35M HC2H3O2 (WEAK ACID) does not dissociate completely. Its Ka = 1.8x10^-5 [H+] = sqrt[(Ka...
Monday, September 14, 2009 at 10:12am by GK

Chemistry
Given a diprotic acid, H2A, with two ionization constants of Ka1=3.9E-2 and Ka2=5.9E-8. Calculate the pH and molar concentration of each protonated form for a 0.135 M solution of: (a) H2A (b) NaHA (c) Na2A
Saturday, July 21, 2012 at 12:04am by Jo

Chemistry
calculate the ph of a solution that results from titrating 0.0500 moles of cyanic acid to the equivalence point with an equal number of moles of OH-, if the final volume of the solution is 150 ml ka= 3.50 * 10^-4
Friday, April 6, 2012 at 11:13pm by Tasneem

Chemistry
Calculate the pH after 0.13 mol of NaOH is added to 1.00 L of the solution that is 0.57 M HF and 1.13 M KF. I got the answer of 3.66 to 3 sig figs, but it's wrong. Can you please tell me what I did wrong? -Thanks
Sunday, March 27, 2011 at 3:02pm by Katrina

science
Calculate the pH of a solution created by mixing 200.0 mL of 0.400 M acetic acid and 200.0 mL of 1.00 M sodium acetate. Hint: The instant the two solutions are mixed what are the initial concentrations of each?
Monday, February 14, 2011 at 2:43am by Bruce

chemistry-confirm please
Only a chemist can be trusted with the combination to the safe containing a ton of money. The combination is the pH of solution A, followed by the pH of solution C. (for example: is the pH of solution A is 3.47 and the pH of solution C is 8.15 the combination to the safe is 3-...
Sunday, May 25, 2008 at 2:51pm by Tom

AP CHEMISTRY
You know acid + water ionizes to give H3O^+ so take the H3O^+ out and see what's left. H3PO4 + H2O ==> H3O^+ + H2PO4^- Then Ka1 = (H^+)(H2PO4^-)/(H3PO4) For the pH. The pH when (H2PO4^-) = (H3PO4). Note one is in the numerator, the other is in the denominator, they ...
Wednesday, February 15, 2012 at 5:05pm by DrBob222

chemistry
solution The hydrogen ion concen.(H+),of the acid is 0.25moldm3 ie(H)=0.25 but ph=-log{H+} ie pH=-Log{0.25} =-log{2.5*10`} =-0.398+1=0.602 but pH+pOH=14 i.e 0.60+pOH=14 ^pOH=14-0.60 =13.40
Thursday, March 10, 2011 at 5:56am by peter onoriode

acid vs base
Calculate the pH of a solution that obtained by diluting 0.015 mol acetic acid with water to 250 cm3 (the Ka - value for acetic acid is 1.74 x 10-5 M).
Friday, February 18, 2011 at 12:36pm by Anonymous

chemistry
Calculate the hydronium ion concentration and pH in a 0.037 M solution of sodium formate, NaHCO2. hydronium ion concentration i dont understand these
Wednesday, March 6, 2013 at 5:01pm by sara

chemistry
Calculate the pH of a solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M benzoic acid (Ka = 6.5 x 10 -5
Tuesday, March 15, 2011 at 2:08am by haley

Chemistry
A 50.0 mL sample of 0.10 M pyridine, C5H5N, is titrated with 0.2 M HBr. Calculate the pH to one decimal place when the following volumes of titrant have been added. 0.00 mL a) 0ml b)17ml c)25ml d)40ml
Thursday, March 7, 2013 at 8:03pm by Katie

chemistry
Calculating final concentrations. Your instructor asks you to add the specified quantities of 2M Tris pH 8.0 buffer to 140 ml of distilled water. Calculate the final concentration and dilution factor of each solution. a)10ml b)20ml c)140ml
Monday, August 27, 2012 at 9:25pm by anonymous

chem
If a neutral solution of water, with pH = 7.00, is heated to 50 deg C , the pH drops to 6.63. Does this mean that the concentration of [H+] is greater than the concentration [OH-]of ?
Monday, July 2, 2012 at 11:25pm by greeny

CHEMISTRY!!!!
You may be expected to derive the equation for calculating the pH of a 0.1M soln of NaHO3. The shortcut equation is (H^+) = sqrt(k1k2) or pH =1/2(pK1 + pK2)
Monday, March 5, 2012 at 3:45pm by DrBob222

chemistry
All you need to do is to substitute into the pH equation. pH = -log(H^+). HCl is a strong acid, it ionizes 100%; therefore, (HCl) = (H^+)
Tuesday, February 28, 2012 at 8:21pm by DrBob222

Chemistry
Can someone tell me if I am doing this problem right or if I need to start over? Thanks. pH = -log [H+] = -log (0.10) =1 The pH of 0.10M HCI solution is 1.
Thursday, January 31, 2008 at 4:53pm by Lisa

chemistry
Calculate the pH of a buffer using dihydrogen phosphate and it's conjugate base. The concentration of weak acid is 0.23 M and the conjugate base concentration is 1.19 M
Wednesday, April 3, 2013 at 10:11am by Anonymous

Chemistry
Calculate z pH of a buffer solun containing o.1 M acetic acid & 0.1 M solun of sodiumacetate when 1 mL of 0.1M HCl is added to 100 mL of buffer .
Tuesday, December 6, 2011 at 2:39pm by Ethio

Chemistry help pliz
continued from above calculate the initial pH of the acetic acid-sodium acetate solution above.The pKa of acetic acid is 4.76
Thursday, September 22, 2011 at 6:41am by Petty

Chemistry
Calculate the pH at 298K of solutions having the following ion concentrations? A. [H+]=1.0 x 10^-4M B. [H+]=5.8 X 10^-11M for A do you subtract 1.0 X 10^-14 from H+]=1.0 x 10^-4M
Monday, March 8, 2010 at 9:27pm by Anonymous

Analytical Chemistry
H3O+= e^-pH+-error = e^-pH * e^-+error =e^-3.72 * e^+-.03
Monday, January 28, 2013 at 10:16pm by bobpursley

Chemistry
pH = -log(H^+). Then pH + pOH = pKw = 14 Solve for pOH.
Wednesday, February 9, 2011 at 11:46am by DrBob222

Chemistry
Calculate the pH at the equivalence point for the titration of 0.200 M methylamine (CH3NH2) with 0.200 M HCl. The Kb of methylamine is 5.0× 10–4.
Monday, March 11, 2013 at 9:23pm by KB

chemistry
Mn(OH)2 ==> Mn^+2 + 2OH^- Ksp = (Mn^+2)(OH^-)^2 You know Ksp and Mn, calculate OH^- and from there pOH, then pH. Post your work if you get stuck.
Friday, December 18, 2009 at 2:57pm by DrBob222

Help Chemistry
Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the ...
Tuesday, December 7, 2010 at 11:01am by Jessica

Chemistry
..........RNH2 + HOH ==> RNH3^+ + OH^- initial...0.1..............0........0 change.....-x..............x........x equil.....0.1-x.............x........x Kb = (RNH3^+)(OH^-)/(RNH2) 6.4E-4 = (x)(x)/(0.1-x). x^2 = 6.4E-5 if we make the assumption that 0.1-x = 0.1. Then x...
Saturday, November 26, 2011 at 8:14pm by DrBob222

AP Chemistry
Consider 67.0 mL of a solution of weak acid HA (Ka = 1.00 10-6), which has a pH of 4.500. What volume of water must be added to make the pH = 5.000?
Tuesday, February 7, 2012 at 7:19pm by Bill

CHEM HELP...PLEASE!!
Sorry, there's one thing I don't understand. If an acid is being added to a buffer solution, shouldn't the pH decrease? By following your method, the answer I'm getting is greater than the original pH.
Monday, March 2, 2009 at 11:21am by Kat

Chemistry
Calculate the pH when 39.0mL of 0.321 of HA is mixed with 39.0mL of 0.321M NaOH where HA is a monoprotic weak acid with Ka= 7.5x10^-5 M ?
Saturday, March 24, 2012 at 6:53pm by Jematormal91

college
Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8*10^-5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant.
Monday, June 21, 2010 at 9:07am by Syra

Chemistry
Consider the titration of 50.0 mL of 0.20 M NH3 (Kb = 1.8x10^-5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant.
Wednesday, October 7, 2009 at 7:55am by Anonymous

chemistry
the concentration of OH ions in a household ammonia cleaning solution is0.0035M. Calculate the concentration of H ions. would it be pH=-log (.0035)??? or Kc=1/.0035???
Thursday, April 10, 2008 at 3:10pm by david

chemistry
Are both of these NaOH? If so, calculate mols of 1, mols of the other, add mols, and divide mols/L(total volume) = molarity. Then pOH = -log (OH^-) and pH + pOH = 14.
Friday, November 16, 2007 at 6:14pm by DrBob222

Chemistry
A factor of 10. Concn 0.1 M acidity = 10^-1 & pH = 1 Concn 0.01 M acidiity = 10^-2 & pH = 2 Concn 0.001 M acidity = 10^-3 & pH = 3
Sunday, July 11, 2010 at 9:38pm by DrBob222

A few chemistry
I got the rest of the homework, but these are confusing me so much...ugghhhh. 1. The pH of a .400 M solution of iodic acid, HlO3, is .726 at 25 degrees C. What is the Ka(acid constant) at this temperature? 2. The pH of a .150 M solution of HClO is found to be 4.55 at 25 ...
Thursday, March 22, 2007 at 10:12pm by Trish

Chemisty
Calculate the \rm pH of a 0.10 M solution of hydrazine, \rm N_2H_4. K_b for hydrazine is 1.3\times 10^{-6}.
Friday, June 14, 2013 at 11:14pm by Karlie

Chemistry
A buffered solution is made by adding 48.6 g C2H5NH3Cl to 1.00 L of a 0.77 M solution of C2H5NH2. Calculate the pH of the final solution. (Assume no volume change. Assume that all solutions are at 25°C.)
Wednesday, March 13, 2013 at 2:47am by Margaret

Chemistry
A buffer is prepared by mixing 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF (Ka = 6.8x10^-4) Calculate the pH of this buffer after 5.0 mL of 0.05 M HCl is added.
Sunday, April 17, 2011 at 4:20pm by Sam

Biochemistry
The KOH and HNO2 exactly neutralize each other and the pH at the equivalence point is the pH of the hydrolyzed salt. It has a concn of 0.1M x (100 mL/200mL) = 0.05M ............NO2^- + HOH ==> HNO2 + OH^- initial.....0.05.............0.......0 change.......-x...
Tuesday, March 27, 2012 at 2:22pm by DrBob222

AP chemistry
1). In a titration 20 mL of 0.100 M of HCl is added to 50.0 mL of 0.150 M of ammonia. A). What is the pH of NH3? B). What is the pH of the resulting solution? HELP :(
Thursday, March 21, 2013 at 5:52pm by Amanda

ChemB
A forming acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addition? Explain. A) HCl B) NaBr C) NaCHO2 D) KCl
Monday, March 12, 2012 at 2:12am by ALISON

SCIENCE
What are the units you are using for pressure? mm of mercury? atmospheres? pascals? I don't see how you can infer a pH from a vapor pressure. Are you sure the number 7 is not already a pH?
Monday, February 7, 2011 at 2:07am by drwls

the pH scale and neutralisation
Hi peeps im 11 and i desperately need help in the pH scale. pleas help me!!!!!!!!!1 c ya lataar hunn bunns xx
Saturday, November 4, 2006 at 5:56am by Anusheh Yunus

Science
The question is: What would happen if you tested bleach with a pH indicator and why? I know that it would turn out with a pH of approx. 12, but I have no idea why. Help please?
Monday, October 12, 2009 at 10:08pm by Amy

chemistry
If the pH = 5.4 then 5.4 = -log(H^+) -5.4 = log(H^+) (H^+) = 3.98 x 10^-6 I didn't work through all the numbers to see if they match up but it doesn't matter what they are. If the pH is 5.4, then (H^+) is defined by that and nothing else.
Thursday, April 17, 2008 at 3:04pm by DrBob222

Chemistry
Given that the pKa for Acetic Acid is 4.77, calculate the expected pH of the buffer solutions using the Henderson-Hasselbalch equation and the concentrations of Acetic Acid and Acetate added to the 250 ml Erlenmeyer flask
Friday, March 18, 2011 at 8:10pm by M_Joe

chemistry
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3CH2CH2COOH with 0.1000 M NaOH after 26.5 mL of the base have been added. Ka of butanoic acid = 1.54 x 10-5.
Sunday, October 31, 2010 at 8:41pm by karla

Chemistry
Hi, I'm trying to solve some chemistry problems, like the ones my teacher says will appear on our exams. The problem reads like this: What is the hydrogen conentration in a bleach sample that register 9.55 using a pH meter? My Attempt: Since this sample register a 9.55 on ...
Monday, December 13, 2010 at 10:45pm by Cliff

Chemistry
This is probably easier then my making it but... Calculate the ph of a forming acid solution that contains 1.35% forming acid by mass. Assume a density of 1.01g/ml for the solution.
Friday, February 24, 2012 at 6:36pm by L.Bianchessi

chemistry
hi kinda stuck :) 100.0 ml of 0.100 M H2NNH2 (kb =3.0 x10^-6) is titrated by 0.200M calculate PH after adding the following volumes of HNO3 a 0 b 25.0 ml c 50.0 ml d 60.0 ml ----------------------------------------- A) N2H4 + HNO3 --> N2H5+ + NO3- .100 0 0 3.0 x 10-6= ...
Sunday, July 26, 2009 at 2:14am by Jim_R

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

biochemistry with more info that was needed
okay, this is what I have so far and now don't know how to finish. I used TRIS. pH=8.30+log(121.1/157.6) pH=8.19 Note: TRIS (Trizma base) MW= 121.1 TRIS-HCL MW= 157.6 (I hope I am using the correct things) After I got the pH, I got stuck on how to finish the problem.
Sunday, January 27, 2008 at 5:35pm by stew

chemistry-Buffer Q
Yes, you would have concn BUT M = moles/L so if you know moles and M you can calculate L and convert to mL. I think you have the right idea; you just quit too soon. moles NH3 = 1.74/17.03 = ? moles (NH4)2SO4 = 4.19/132.14 = ? and that x 2 = about 0.0628 ...........NH3 + H...
Monday, November 14, 2011 at 6:47pm by DrBob222

economics
a monopolist, has a total cost curve given by TC = 5Q + 15. He sets two prices for his product, a regular price, PH, and a discount price, PD. Everyone is eligible to purchase the product at PH. To be eligible to buy at PD, it is necessary to present a copy of the latest ...
Friday, January 8, 2010 at 5:53am by v

chem
I understand how to get the pH before titration and how to get the volume. From my understanding to get the pH before titration i just multiply the ka and the weak acid concentration then i get the square root. I then get the negative log of the square root and i got 5.8 as ...
Monday, March 1, 2010 at 11:38pm by simi

pH scale
If a base is added to water, the pH will increase, decrease, stay the same, or increase sometimes and decrease sometimes. I have asked several friends and the two answers I get is increase from 3 of them and stay the same from 2 of them. I am confused. And so are your friends...
Wednesday, January 17, 2007 at 3:43pm by Jacob

chem
Calculate molarity of KOH solution. That is 1.14 g/mL x 1000 mL x 0.15 = approximately 175 grams KOH. So mols KOH = 175/56 = about 3 M. Now go to what you want to prepare. You want pH = 11.60 which is pOH or 2.40 or (OH^-) = about 0.004 M. Now mL(soln 1) x M(soln 1) = mL(soln ...
Monday, February 16, 2009 at 11:48pm by DrBob222

Analytical Chemistry
First determine the volume for the equivalence point. For zero mL you have a solution of KOH only. Since that is a strong base and is 100% ionized, solve for OH and convert to pH. At the equivalence point, the pH is determined by the hydrolysis of the salt. At all points ...
Saturday, November 26, 2011 at 4:36pm by DrBob222

Chemistry
Calculate the H3O+ ion concentration and the pH at the equivalence point when 45.0 mL of 0.4000 M NH3 is mixed with 45.0 mL of 0.4000 M HCl. Ka=5.6x10-10
Sunday, April 21, 2013 at 1:40pm by john

chemistry
A buffer solution was prepared by mixing 442 mL of 0.181 M NaOCl and 139 mL of 0.421 M HOCl. Calculate the pH of the solution given that Ka (HOCl) is 3.2 x 10-8.
Sunday, March 18, 2012 at 7:39pm by cathy

Chemistry
Calculate the pH at the equivalence point of 25.0 mL of a 0.100 M acetic acid, CH3COOH, titrated with a 0.100 M sodium hydroxide, NaOH. Ka of acetic acid is 1x10^-5
Sunday, April 11, 2010 at 12:53pm by Anonymous

AP Chemistry
In the titration of 50.0 mL of 1.0 M CH3NH2 (kb=4.4 x 10^-4), with 0.50 M HCl, calculate the pH a) after 50.0 mL of 0.50 M has been added b) at the stoichiometric point.
Sunday, March 29, 2009 at 11:41pm by some kid

chemistry
The Henderson-Hasselbalch equation for buffers is pH = pKa + log (base/acid) If you want (base) = (acid), then log base/acid is log 1 and that is zero; therefore, pH is pKa. Just look up the pKa for the acid of each pair and that will be the pH.
Sunday, October 9, 2011 at 1:43pm by DrBob222

Chemistry
14-pH = pOH From the pOH, you can calculate [OH-] raising 10 to the opposite pOH power. [OH-]=10^(-pOH)
Sunday, April 1, 2012 at 10:48am by vox

Chemistry
What volume of a 0.22mol/L hydrochloric acid solution is needed to cause the pH of 25.00mL of a 0.15mol/L lithium hydroxide solution to have a pH that s equal to 7.00
Saturday, February 16, 2013 at 9:42pm by Amy

Chemistryr
Add 0.40 g of NaOH to 50.0 mL of 0.10 M HCOOH, and find approximate pH. No volume change, Ka HCOOH=1.8x10^-4. I get pH 8. Right?
Thursday, May 6, 2010 at 6:16pm by Jim

AP Chemistry
i found the pH to be 9.75, i don't know if i did it right, Assuming i did it right, there is another question stating what is the pH of the buffer after 90.0mL of 2.00M HCL are added?...
Sunday, April 11, 2010 at 3:51pm by Yamani

chemistry-acids and bases
determine how many mL's of a monohydroxic base with a pH of 9 is needed to neutralize 50 mL of a monoprotic acid with a pH of 2. I do not understand what to do. can someone please help?
Monday, May 25, 2009 at 3:53pm by jackie

AP Chem
Calculate the correct volumes of the 0.1M acetic acid solution and the 0.1M sodium acetate solution needed to make 50mL of a buffer solution with a pH vaule of 5.00. (Ka = 1.8x10^-5)
Sunday, March 11, 2012 at 5:23pm by Keighley

Chemistry
My chemistry teacher said that the pCO2 value increases during hypoventilation. Why is that? If hypoventilation causes shortness of breath, would that not increase the CO2 concentration, therefore decreasing pCO2? Because if you think about pH, a larger H concentration causes ...
Sunday, March 11, 2012 at 1:12pm by Bobby

chemistry
pH = -log(H^+) and pOH from pH + pOH = pKw = 14.
Tuesday, March 20, 2012 at 3:55pm by DrBob222

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