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: 25,387

Honors Chemistry
1. What is the pH of a solution whose [H3O+] is 1 X 10^ -5 M? 2. What is the [H3O+] concentration of a solution with a pH of 9? 3. What is the pH of a solution whose [H3O+] concentration is 3 X 10^-3 M? 4. What is the pH of a solution with a [H3O+] concentration of 1 X 10^ -12...
Friday, April 6, 2012 at 11:18am by Chris

chemistry
The pH of a solution is 6.0. Explain how the addition of the following substance would alter (or not alter) the pH of the solution. a. HCl b. NaOH c. H20
Monday, January 24, 2011 at 10:58pm by steven

Chemistry
1- Determine the [OH-] and pH of a solution that is .250 M in HCO-3 2- Calculate the [H3O+] and pH of each polyprotic acid solution: a) .125 M H2CO3 b) .125 M H3C6H5O7
Monday, March 14, 2011 at 4:56pm by Joey

AP Chem
A 0.23 M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8.68. Calculate the pH of a 0.23 M chlorobenzoic acid (HC7H4ClO2) solution
Sunday, February 15, 2009 at 11:54pm by Jake

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(Please respond)
I did an experiment to study the effects of changes in conditions on an equilibrium system. The first system was the dissociation of acetic acid. HC2H3O2 -> H^+^ + C2H3O2^-^ <- We had to add 2mL of acetic acid into a test tube and we had to test the pH of the ...
Wednesday, March 14, 2012 at 10:23pm by Hannah

Ph CHEM
A solution is found to contain 1 x 10-4 OH− ions, determine the pH of this solution. I did this problem and got 4 but it is not going in as correct. -log(1*10^-4)=4
Tuesday, November 27, 2012 at 9:31pm by Lara

Chemistry
I have a 40 ml solution of pH 4.36. I need to make this solution at pH 8.5 by adding extra 10 ml of HCl and NaOH. Thanks
Monday, August 6, 2012 at 7:49am by AAA

chemistry
A solution of sodium cyanide NACN has a PH of 12.10. How many grams of NACN are in 425ml of solution with the same PH? Please helps me to solve it for me
Sunday, August 5, 2012 at 1:09pm by Fai

chemistry
explain why you get two different pH values for same solution when calculating and using pH meter of same solution?
Friday, February 11, 2011 at 9:50am by kabelo

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
Calculate the pH range required to separate 99.99% of Cr3+ from Zn2+ by precipitation of Cr(OH)3(s) in a solution that is initially 0.034 M in both Cr3+ and Zn2+. Use the Ksp values from Table 16.2 of Chang and calculate the pH to the nearest 0.01 pH unit. Lowest pH= Highest pH=
Sunday, March 25, 2012 at 5:17pm by Tanner

Chemistry 12
15. The concentration of hydroxide ions in a solution of nitric acid 0.2 M is: a. 2 x 10-14 M b. 5 x 10-14 M c. 5 x 10-7 M d. 2 x 10-1 M 16. Aqueous solutions of strong acids and strong bases: a. are good electricity conductors b. make litmus paper become red c. have a pH of 7...
Monday, December 3, 2012 at 6:58pm by Need Help

Chemistry
I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH. This is my data: Conc.of...
Thursday, July 16, 2009 at 3:36am by Saira

Chemistry
I have a test on monday and I NEED to ace it in order to raise my grade > . < ldsfkjaslkf right now, acids and bases are killing me can somebody help me with these problems? A buffer solution is prepared by mixing the weak base ammonia (Kb=1.77x10^-5) with ...
Saturday, May 15, 2010 at 2:10pm by Kimberlee

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

chemistry
I asked this before, but got no response. A) If you make up a solution of 250 mL of 0.1 M TRIS in the acid form, what will be the pH? B) If you add 2 mL of 1 M NaOH to the solution in part A, what will be the pH? Thanks.
Sunday, February 3, 2008 at 2:43pm by student

chemistry
A) If you make up a solution of 50 mL of 0.1 M TRIS in the acid form, what will be the pH? (pka of TRIS: 8.3, molecular wt: 121.1 g) B) if you add 2mL of 1 M NaOH to the solution, what will be the pH? Thank you.
Saturday, February 2, 2008 at 4:09pm by matt

Chemistry
A solution of acetic acid having a concentration of about 0.2M is to be titrated using 0.200M NaOH. Select an indicator for the titration. what salt will the solution contain at the equivalence point? what is the approximate concentration of this salt at the equivalence point...
Saturday, May 15, 2010 at 2:00pm by Alison

Chemistry, Buffers, pH
Hi could someone please help me in the next 5 minutes with this question: Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show...
Friday, September 26, 2008 at 1:30am by janet

CHEMISTRY/
A student takes a 1.00 mL aliquout of 5.00*10^-4 M HCl solution and dilutes it to the mark with water in a 1000.0 mL volumetric flask. (a)What is the expected pH for the final solution at 25C? (b)What would be the expected pH if this solution were later used at a temperature ...
Sunday, March 20, 2011 at 5:38am by TORI

chemistry
Water in contact with air is acidic due to the dissolved carbon dioxide. Water in equilibrium with the air contains 4.4 x 10^-6% CO2. The resulting carbonic acid, H2CO3,gives the solution a hydrogen ion concentration of 2.0 x 10^-6M, about 20 times larger than that of pure ...
Saturday, March 24, 2007 at 1:06pm by Heather

chemistry
Calculate the pH at the equivalence point for the titration of a solution containing 1250.0 mg of hilariamine (MW = 92.5 g/mol, Kb = 8.1×10−4) with 0.1000 M HCl solution. The volume of the solution at the equivalence point is 175.0 mL. (I got the answer to be ...
Sunday, May 15, 2011 at 8:02pm by vivian

algebra 2
The pH of a solution is given by the formula pH = -log H+ , where H+ is the concentration of hydrogen ions in moles per liter in the solution. Use this formula to solve the problem. Round answer to one decimal place if necessary. Find the pH of a sample of lake water whose [H...
Thursday, July 14, 2011 at 1:59pm by jay

Chemistry
Calculate the change in pH if 0.050 g of solid NaOH is added to 250 mL of a buffer solution that contains 0.80 M NaH2PO4 and 0.17M Na2HPO4. I found the pH of the buffer solution to be 6.54.
Thursday, April 4, 2013 at 6:36pm by Matt

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
how do I find the pH of a buffer solution given that 0.010M NH3 mixed with 0.0030M NH4Cl. Also... a 0.010M HF solution is mixed with 0.030M KF. FIND THE pH of this mixed solution.
Sunday, March 25, 2012 at 9:03pm by Declan

Chemistry
Calculate the pH of a 5.90 10-3 M solution of H2SO4 I have tried doing this as pH=-log[H+] and also by multiplying the Molarity by two because there are two hydrogens and then doing the -log but both ways have gotten me the wrong answer is there something i am missing? same ...
Monday, March 5, 2012 at 9:54pm by Ashley

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
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 HELP PLEASE!!!
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu^2+(aq,1.0M)|Cu(s) what is the pH of the solution if Ecell is 375 mV? I first got .65 as my pH, but it said that it was wrong. ...
Saturday, March 30, 2013 at 9:33pm by clara

chemistry
Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2.
Saturday, April 18, 2009 at 3:05pm by Hannah

Chemistry
3) The pH of a buffer solution made out of 0.20mol/L hydrofluoric acid and 0.30mol/L sodiumfluoride is the same as a buffer solution that is made out of 0.10mol/L of acetic acid and 0.15mol/L of sodium acetate. HF: pH = 3.14 + log(0.3/0.2) = 3.33 HAc: pH = 4.75 + log(0.15/0.1...
Saturday, December 8, 2012 at 2:54pm by DrBob222

chemistry
Adding acid will make it more acid; pH will go down. Adding base will make the solution more basic; pH will go up. Adding water will make the solution more dilute and it will change the pH somewhat (a little more basic making pH go up); how much depends upon how much water is ...
Monday, January 24, 2011 at 10:58pm by DrBob222

Chemistry
Consider a 0.80M solution of HCN. The Ka of HCN is 6.2x10-10. What are the major species in solution? Calculate the pH of this solution. ----------------------------------- Ok, so i took a break, came back, and finished the problem. I have an x value of 2.23x10-5. I took the ...
Tuesday, October 18, 2011 at 2:17am by Kevin

Chemistry
1. What is the pH of a solution whose [H3O+] is 1 X 10 -5 M? 2. What is the [H3O+] concentration of a solution with a pH of 9? 3. What is the pH of a solution whose [H3O+] concentration is 3 X 10-3 M? 4. What is the pH of a solution with a [H3O+] concentration of 1 X 10 -12 M...
Tuesday, March 27, 2012 at 12:21pm by John

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
A solution of sodium cyamide nacn has a ph of 12.10. How many grams of nacn are in 425ml of solution with the same PH Who helps me to solve it for me. Step by step
Sunday, July 29, 2012 at 1:09pm by Fai

Chemistry
1.)Find the PH of a solution with 0.20M NH3 with 0.15M of NH4Cl. 2.)Find PH of a solution with a mixture of 200mL of 0.50M HCHO2 and of 100mL of .50M NaCHO2.
Tuesday, May 1, 2012 at 5:02pm by Chem help me!

Chemistry
Use solution B to solve for the Ka of the weak acid. Use Ka from above to solve for the pH of solution A. That gives you the first 3 numbers of the combination. Use solution C and the Henderson-Hasselbalch equation to solve for the pH of that solution which will be last three ...
Tuesday, May 27, 2008 at 7:38pm by DrBob222

Chemistry
How many mL of a solution of NaOH with pH equal to 1.395 x 101 do you need to mix with pure water to obtain 399 mL of a final solution with pH equal to 9.066 ?
Tuesday, January 17, 2012 at 2:19pm by Summer

chem
I don't think so. Now that I see the question again, I'm wondering if this is a problem with two parts; i.e., the question is asking for the pH of 0.0515 M HCl and for the pH of a separate solution of 0.0762 M NaC2H3O2? And after noticing that there is no volumes ...
Thursday, April 16, 2009 at 2:09pm by DrBob222

Chemistry
NH3 + HCl ==> NH4Cl moles NH3 = M x L = ?? moles HCl = M x L = ?? Determine from the moles you have which reagent is in excess, determine the molarity from M = mole/L and find pH of the resulting solution. I suspect NH3 is in excess and that will produce a buffered ...
Sunday, February 13, 2011 at 11:32pm by DrBob222

chemistry
What is th pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1L of water? What is the molarity of a solution made by dissolving 3.4g of Ba(OH)2 in enough water to make 450mL of solution? Assume that Ba(OH)2 ...
Wednesday, November 18, 2009 at 9:53pm by Taylor

chemistry
a)Calculate the pH of a solution of 0.75 M HNO3, which is a strong acid. b)Calculate the pH of a 1.0 L aqueous solution made from 0.80 mol CH3COOH and 0.20 mol KCH3COO (Ka = 1.8 x 10^-5).
Thursday, May 9, 2013 at 9:36am by alex

chemistry lab
Could someone help me with this? i am tired of it. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01 M: 7.42 pH of ...
Friday, February 1, 2008 at 10:54pm by amanda

Chemistry
see same question how many grams nitric acid HNO3 must be dissolved in 350 ml water to make a solution with pH of 4.5"? or "how many ml of a 4.2M nitric acid solution are required to make 500 ml of solution with pH of 2.9
Sunday, May 12, 2013 at 11:29am by kriti

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
To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a) Calculate the pH of the new solution. b) What becomes the pH if another 20.00 mL of the same acid solution is added?
Friday, February 15, 2013 at 10:49am by faizer

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

Chemistry
A solution that contains 2.047 x 10^-1 M of acid, HA, and 1.808 x 10^-1 M of its conjugate base, A-, has a pH of 4.196. What is the pH after 1.629 x 10^-3 mol NaOH is added to 5.961 x 10^-1 L of this solution?
Saturday, January 21, 2012 at 11:17pm by Summer

chemistry
SALT HYDROLYSIS 1.) Calculate the pH of a 0.24M sodium formate (HCOONa) solution. Kb=5.9x10^-11. 2.) Calculate the pH of 0.25M pyridium chloride (C5H5NHCl)solution. Ka=5.9x10^6.
Thursday, January 20, 2011 at 5:18am by jaycab

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
1. Find the pH of a solution whose [H3O+] is 9.5 X 10^ -8 M. 2. What is the [H3O+] concentration of a solution with a pH of 5.45? 3. What is the pOH of a solution with a [OH -] concentration of 2.97 X 10^ -10 M?
Monday, May 14, 2012 at 12:41pm by kellin

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

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
IN the polystyrene beaker, mix 20mL of 0.1 M Acetic acid and 25mL of 0.1M Sodium Acetate and immediately measure the pH. Remove the electrode and add 5ml of 0.1 M HCl to this buffer. Stir the solution and measure the pH. _______________ INFO: concentration of acetic acid= 0.1M...
Sunday, March 28, 2010 at 5:53pm by Saira

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/pH- Weak Acid
Hi again! I have a new question, Can you help me? Consider 50.0 mL of a solution of a weak acid HA (Ka = 1.00.E-6), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000? My Calculations: To calculate the concentration of x, I take the pH value -&...
Sunday, August 17, 2008 at 6:07am by Mary

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
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
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

Chemistry
3. A chemistry student makes up a 0.10 M solution of NaF(aq) and finds the pH to be 8.09. a. Explain why the presence of F- in this solution affects the pH. b. Write out the acid/base equilibrium equation for the reaction of F- with water. c. Use the measured pH value to solve...
Wednesday, April 4, 2012 at 9:57pm by chamy

chemistry
A 2.5 g sample of NaOH (Mw = 40.00) was dissolved in water to give a solution of final volume 250 cm3. (i) With reasons, state whether NaOH is a strong or a weak base. Give the conjugate acid of NaOH and decide whether this conjugate acid is acid, alkaline or neutral. (ii) ...
Sunday, April 21, 2013 at 10:01am by LUx

chemistry
what is the pH of a solution that is .15 M in HOCl and .25 M NaOCl after .05 mol HCl/L has been bubbled into the solution? this is what I did: HOCl + H2O ----> H3O+ + OCl- .15 .25 -.05 +.05 --------------------------- .1 .30 3.5E-8=[H3O][.3]/[.1] H3O= 1.167E-8 pH= -log(...
Tuesday, November 23, 2010 at 11:44am by Audrey

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-science
A 500 ml buffer solution contains .2M Acetic acid and .3M sodium acetate. Find the pH of the buffer solution after adding 20 ml of 1M NaOH, what is the pH? (pka = 4.74)
Friday, April 30, 2010 at 3:22am by jess

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

biology
another way to afect the enzyme is lowering the pH of the solution. However, lactase is supposed to be able to work in the stomack. Would lowering the pH of the enzyme solution affect the enzyme? Why or why not?
Friday, November 11, 2011 at 11:12am by sara

Chemistry
What will be the pH of: (a)10.0cm3 of an aqueous solution of 0.001mol dm^-3 nitric aicd, HNO3 (aq)? (b)100cm3 of an aqueous solution of 0.001mol dm^-3 nitric aicd, HNO3 (aq)? (c)0.02mol dm^-3 of potassium hydroxide solution, KOH (aq)? For (a) I got 2, (b) 1 and (c) 12.31. I am...
Tuesday, November 17, 2009 at 3:47pm by Anonymous

Chemistry
1.What is the pH of a solution containing 0.042 M NaH2PO4 and 0.058 M Na2HPO4 ? The pKa of sodium phosphate is 6.86. pH = 6.86 + log [0.058] / [0.042]; pH = 6.86 + 0.14; pH = 7.00 That is my answer to the above question. The following question is what I am having trouble with...
Sunday, January 27, 2013 at 11:00pm by Blake

Chem
Consider a solution that contains both C5H5N and C5H5NHNO3. (Kb for pyridine, C5H5N, is 4.0 x 10^-4) (a) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 4.50. (b) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 5.00.
Tuesday, April 7, 2009 at 12:36am by Fred

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

Biology
In a lab experiment, we experimented with 1% glucose solution and Sorenson's solution to determine pH levels and whatnot; the other part of the lab was to determine which one, if either, was a buffering solution. According to the notes my instructor gave us, a buffers are ...
Monday, January 28, 2013 at 1:10pm by Emily

chemistry
A solution has H+ = 5.0 ´ 10–5 M. Assume temperature of the solution is 25 Centigrade.The pH of this solution is?
Tuesday, June 12, 2012 at 10:07pm by sidd

chemistry
Will this solution form a buffer? 100 mL of .10 M NH3; 100 mL of .15 M NH4Cl Work: NH3= .01 moles NH4Cl= .015 moles .... not sure what else to do. I think we use the H-H equation, but I don't know how to find pKa, or even what pKa is. This should give the pH of the ...
Friday, March 19, 2010 at 7:41pm by Vanessa

Chemistry II
If 15.0 mL of 1.2e-4 mol/L HI is added to 26.0 mL of 9.2e-4 mol/L HI, what is the pH of the solution? M x L = mols. Calculate mols for solution 1, do the same for solution 2, add mols together and divide by total liters. That will be the new molarity. Then pH = -log(Molarity)
Tuesday, April 24, 2007 at 9:39pm by Jayd

biochemistry
The pH of 0.02M solution of a weak acid was measured at 7.6. What is the [OH-] in this solution? B) The Ka for benzoic acid is 6.4 x 10-5M. 150 ml of 0.1 M NaOH is added to 200 ml of 0.1 M benzoic acid, and water is added to give a final volume of 1 L. What is the pH of the ...
Friday, September 21, 2012 at 9:38am by Emma

Chemistry(Please check answers)
1) The Ka for acetic acid is 1.8e-5. What is the pH of a 3.18M solution of this acid? I did 1.8e-5 = x^2/3.18 x=sqrt 1.8e-5 X 3.18 = 7.56e-3 pH=-log(7.56e-3) = 2.12 The pH is 2.12 2) At 25 degrees celsius, the pH of a 1.75M NaCN solution (the Ka for HCN is 4.0e-10) is ? 4.0e-...
Sunday, April 1, 2012 at 3:40pm by Hannah

Chemistry
If 100mL of a 0.10M NaOH solution is added to 75mL of a 0.15 HCl solution, then what is the pH of the resultant solution?
Wednesday, August 22, 2007 at 10:10pm by Bert

Chemistry
1.Calculate the pH of a solution prepared by mixing 20mL of the .07222M aspirin solution with 10mL of .2M NaOH. 2. Calculate the pH for the titration of 40mL of .1M solution of C2H5NH2 with .1M HCl for a)0 mL added and b)20 mL added c)40 mL added d)50mL added. Kb= 6.4x10^-4
Saturday, November 26, 2011 at 8:14pm by Jessica

analytical chemistry
A solution containing both Fe 3+ and Al 3+ can be selectively analyzed for Fe 3+ by buffering to a pH of 2 and titrating with EDTA. Th e pH of the solution is then raised to 5 and an excess of EDTA added, resulting in the formation of the Al 3+ - EDTA complex. The excess EDTA ...
Saturday, May 4, 2013 at 9:36pm by jody

chemistry
A solution containing both Fe 3+ and Al 3+ can be selectively analyzed for Fe 3+ by buffering to a pH of 2 and titrating with EDTA. Th e pH of the solution is then raised to 5 and an excess of EDTA added, resulting in the formation of the Al 3+ - EDTA complex. The excess EDTA ...
Tuesday, March 26, 2013 at 1:37pm by jody

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

chemistry
a saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.5. What is the hydronium concentration of the solution? is the solution acidic or basic?
Tuesday, July 14, 2009 at 7:10pm by angela

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
What is the pH of an aqueous solution of 0.10 M NaHC(3)H(2)O(4)? Answer: 10.9 What I did: NaHC(3)H(2)O(4) + H(2)O--><-- Na + H(2)C(3)H(3)O(4) + OH H(2)C(3)H(3)O(4) is Malonic acid with a Ka value of 1.5*10^(-3) initial-change-equilibrium (i.c.e) table results: (x...
Saturday, July 30, 2011 at 7:02pm by pH levels

biology
If the pH of a sample was 3 how many times more acidic is it than a solution with a pH of 6?
Sunday, November 2, 2008 at 8:13pm by Astrid

Gen CHEM 2
This is all they gave me: You need to produce a buffer solution that has pH 5.28. You already have a solution that contains 10 millimoles of acetic acid. How many millimoles of solid sodium acetate will you need to add to this solution? The of acetic acid is 4.74. Then they ...
Monday, February 11, 2008 at 9:42pm by Jessica

biology
What changes occur when a solution goes from ph 5 to ph 8
Monday, January 23, 2012 at 7:47pm by Littlerakka

Chemistry
pH=1/2pKa-1/2(log (C) first solution pH should be 4.17
Monday, April 30, 2007 at 8:37pm by share

Chemistry
The pH of a NaHCO3 solution is independent of the concn. pH = 1/2(pk1 + pk2)
Tuesday, April 13, 2010 at 9:51pm by DrBob222

Survey of the sciences
When the hydronium ion comcentration of a solution equals 1 mole per liter, what is the pH of the solution? Is the solution acidic or basic?
Wednesday, February 9, 2011 at 5:12pm by Stephanie

chemistry
A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.84 M solution of NH3. Calculate the pH of the final solution
Tuesday, August 10, 2010 at 3:14pm by chris

Chemistry Acid/bases
The concentration of H2SO4 in a solution is 3.20 10-6 M. Assume the acid dissociates completely in solution. What is the [H3O+] in the solution? What is the [OH-] in the solution? What is the pH of the solution? What is the pOH of the solution? OK SO I KNOW HOW TO DO THESE ...
Tuesday, February 10, 2009 at 8:11pm by Spencer

Chemistry
.12M Lactic Acid (HC3H5O3, Ka=1.4x10^-4) is mixed with .10M NaC3H5O3 to form 1.00L solution. A. Calculate the pH of the solution after the addition of 50.0mL of 1.00M NaOH. B. Calculate the pH of the solution after the addition of 120.0mL of 1.00M NaOH.
Sunday, March 28, 2010 at 12:16pm by Emma

College Chemistry
Calculate both [H30] and [OH-] for a solution that is: pH=5.50 ph=7.00
Sunday, April 26, 2009 at 10:15pm by Gayla

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