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April 16, 2014

Search: Calculate the pH of a solution made by mixing 50.0 mL of 0.040 M NaOH and 25.0 mL of 0.10 M HClO.

Number of results: 85,241

Chemistry
Consider the titration of 100.0 mL of 0.260 M propanoic acid (Ka = 1.310−5) with 0.130 M KOH. Calculate the pH of the resulting solution after each of the following volumes of KOH has been added. (Assume that all solutions are at 25°C.) (a) 0.0 mL (b) 50.0 mL (c) 100.0 ...
Wednesday, March 13, 2013 at 2:56am by Margaret

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)? Complete the table below: Note: Make simplifying assumptions, do not use the quadratic formula. What are the pH ...
Sunday, October 30, 2011 at 9:10pm by Billy

chemistry
A 20.1 mL sample of a weak monoprotic acid, HX, requires 50.0 mL of 0.060 M NaOH to reach the equivalence point. After the addition of 30.0 mL of NaOH, the pH is 4.90. What is the Ka of HX?
Sunday, March 27, 2011 at 10:46pm by Anonymous

Chemistry
1.CALCULATE pH of 1.0 L 0.010 M ascetic acid and 0.50 L 0.010 M NaOH. 2. Calculate pH of 1.0 L 0.010 M NaOH and 0.500 L 0.010M HCl Buffer help?
Thursday, March 15, 2012 at 8:58pm by ALISON

chemistry
Hello, im having major issues with this problem...A 100.0-mL solution of 0.017 M CH3COOH (Ka = 1.8 10-5) is titrated with 0.025 M NaOH. Now, I've gotten some the answers all ready (right answers have *)....but three of them are wrong, can someone tell me what to do? 1.) ...
Wednesday, October 12, 2011 at 9:44pm by A person

chemistry
Please let me know if my answer to the following question is correct. Question: 25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L acetic acid. Calculate the pH of the solution. Answer: Add 25 mL and 21 mL to get 46 mL. Add 0.45 mol/L and 0.35 mol/L to ...
Tuesday, April 15, 2008 at 4:55pm by Abigail

AP Chemistry
help with acid/bases If the pH at 50.0 mL of NaOH added is 4.0 and the pH at 150.0 mL of NaOH added is 8.0, determine the values Ka1 and Ka2 for the diprotic acid. Ka1 i dotn know how to start, please help!
Wednesday, March 11, 2009 at 12:50am by Amy

chemistry
The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is ?.
Tuesday, November 23, 2010 at 7:00am by ben

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 6:01am by Mary

quantitative chemistry
Consider a solution made by mixing 500.0 mL of 0.04182 M Na2HAsO4 with 500.0 mL of 0.03645 M NaOH. Complete the mass balance expressions below for Na and arsenate species in the final solution. There are 4 arsenate species, but I only got three of them. I am unsure of what the...
Friday, March 22, 2013 at 2:23pm by Jackie

Chemistry
14-pH=pOH=14-10.5=3.5 pOH=-log[OH-]=3.5 10^-(pOH)=10^-(3.5)=OH concentration in M 4.40L*(OH concentration in M)= moles of OH moles of OH*(39.997 g/mol)= mass of NaOH needed mass of NaOH needed Since 15% is 0.15g of NaOH/g of solution, solving for g of solution mass of NaOH ...
Sunday, March 17, 2013 at 1:58pm by Devron

chemistry pls help
If 10.0 mL of 1.0M HCl is added to 90 mL water, what is he concentration of the new solution? What is the pH of this solution? If the solution is titrated by 0.500M Ca(OH)2, how much volume (ml) of NaOH necessary? Need help pls.
Saturday, December 8, 2012 at 12:37am by Emmy

Chemistry
20 ml of 0.1 M acetic acid was mixed with 25 ml of 0.1 M Sodium Acetate. The pH was measured to be 4.43. 5 ml of 0.1 M Sodium Hydroxide was added to the buffer and the pH was measured to be 4.60. Calculate the pH of the buffer before and after the addition of NaOH.
Monday, March 25, 2013 at 7:17pm by Annie

CHEM-102
Calculate the pH of a solution prepared by mixing 10.00mL of 0.50M NaOH and 20.00mL of 0.50M benzoic acid solution. (Benzoic acid is monoprotic; its ionization constant is 6.7x10^-5).
Sunday, March 27, 2011 at 5:55pm by Christian

General Chem
What do you call a solution that is maid by mixing solid Na2S2O3 5H20 with NaOH? Also, what is the complete balanced equation for mixing the above solution with an aqueous solution of NaClO? Thanks anyone!
Wednesday, June 22, 2011 at 7:14pm by Mark

Chemistry
What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 4.40 L of an NaOH solution with a pH of 10.5?
Sunday, March 17, 2013 at 1:58pm by Emma

Chemistry 2
A solution of NaOH (aq) contains 8.2 grams of NaOH(s) per 100.0 mL of solution. Calcualte Ph and POH at 25 degrees celsiuis
Friday, February 21, 2014 at 2:30pm by Jason

chemistry
If you made up a solution of NaOH by adding 0.010 mole of solid NaOH to 1.0 liter of distilled water, what would be the pH of the solution?
Tuesday, December 18, 2012 at 3:15pm by Monica

College chemistry
A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.70 M solution of NH3. Calculate the pH of the final solution. (Assume no volume change.)
Wednesday, March 10, 2010 at 4:19am by Nikita

Chemistry
Assignment  Calculate the pH, pOH, [H+], and [OH] for each of the following solutions. Show all work. (10 Points) Solution Composition of Starting Materials 1 0.10 M acetic acid 2. 5 mL 0.10 M acetic acid + 5 mL wa 3 1 mL 0.10 M acetic acid + 99 mL water 4 5 mL...
Monday, October 11, 2010 at 12:24pm by Brian

pH- really hard one
What is the pH of the solution created by combining 1.00 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)? NaOH + HCl ==> NaCl + H2O So all the NaOH is neutralized leaving NaCl, which will not affect the pH either way, ...
Sunday, April 15, 2007 at 7:39pm by Christine

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 1:49pm by David

Chemistry
Q1: You wish to prepare a buffer solution with pH = 11.10. What volume of 6.0 M HCl would you add to 500 mL of 0.10 M (C2H5)2NH to prepare the buffer? You may assume that the solution’s volume remains constant. Q2: What is the resulting pH when 20 mL of 0.20 M NaOH is added to...
Sunday, February 24, 2013 at 2:16pm by Anonymous

chemistry
2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate the pH of the solution formed by adding 10...
Sunday, March 25, 2012 at 6:06pm by bob

chemistry
enzoic acid is a weak monoprotic acid with Ka = 6.5×10-5 M. NaOH(s) was gradually added to 1.00 L of 8.66×10-2 M benzoic acid. 1. Calculate the pH of the solution before the addition of the base. 2. Calculate the pH of the solution after the addition of 5.20×10-2 mol of NaOH(s).
Tuesday, March 25, 2014 at 9:14pm by bekah

chemistry- some help plzz totally lost on this one
Start with 100 mL HCl, left with 83.0 means you have added 17.0 mL HCl to the beaker. Start with 100 mL NaOH, left with 88 mL means you have added 12 mL NaOH. Calculate moles HCl and moles NaOH added and subtract to determine the excess acid in the beaker. Then use pH 2.70 to ...
Monday, July 13, 2009 at 1:15pm by DrBob222

Chemistry
What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 25.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb= 1.8 × 10-5 for NH3.
Monday, April 29, 2013 at 3:35am by John

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

Chemistry- please help
OK. Boil the water, add about 25 mL of the cooled water to the 100 mL volumetric flask containing the solid NaOH, let the NaOH dissolve, then let the whole thing cool. Finally, dilute to the 100 mL mark. How to prepare carbonate free NaOH. Prepare a concd solution of NaOH by ...
Saturday, September 18, 2010 at 8:27pm by DrBob222

chemistry
A buffer is made by adding 0.300 mol HC2H3O2 and 0.300 mol NaC2H3O2 to enough water to make 1.00 L of solution. The pH of the buffer is 4.74 . Calculate the pH of this solution after 0.020 mol of NaOH is added.
Thursday, December 10, 2009 at 10:59pm by Ericka

Chemistry
Construct the data chart and the pH curve for the titration of 25 mL of 0.1 M CH3COOH with 0.1M NaOH. Add the titrant 1 mL at a time and calculate the pH after each addition
Tuesday, April 19, 2011 at 12:28am by Jake

Chemistry
Calculate the Concentration of Ni2+ in a soltion which prepared as mixing 50.0ml 0.0300 M Ni2+ and 50.0mlml 0.0500 M EDTA at pH= 3 At pH=3 , α4= 2.5x10-11 KNiY=4.2x1018
Sunday, April 15, 2012 at 9:28am by David

chemistry
A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128 M HClO_4_ to reach the equivalence point. What is the volume of the NaOH solution?
Thursday, March 8, 2012 at 10:40pm by Savannah

chem
What is the pH of the solution created by combining 2.40 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)? I understand how to find the pH for the NaOH + HCl solution. However, I'm not sure how to find it for HC2H3O2. I ...
Monday, May 2, 2011 at 8:10pm by Anonymous

Algebra
A saline solution was made by mixing 11 ml of a 36% saline solution and 6 ml of a 53 % saline solution. How do I find the consentration of the new mixture?
Monday, October 18, 2010 at 5:49pm by Hannah

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
the density of a certain aqueous solution is 1.17g/ml, and the solution is 3.57% by mass NaOH. how many mL of this solution would you need to use in order to prepare 100.0 mL of .150 M NaOH solution?
Monday, September 6, 2010 at 6:46pm by zahra

chemistry
1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH ...
Tuesday, October 25, 2011 at 10:55pm by djella

chemistry
What is the pH of the solution that results from mixing the following four solutions together? (1) 150. mL of 0.250 M NaCl (2) 300. mL of 0.200 M HCl (3) 100. mL of 0.050 M HNO3 (4) 450. mL of 0.200 M NaOAc any help is greatly appreciated!
Sunday, March 7, 2010 at 1:15am by Daniel

chemistry
A solution is prepared by mixing 5.00 grams of compound Z (molar mass 15.00 g/mol) in 100.0 ml of water. The density of the solution is 1.09 g/ml. Calculate the molarity of the solution
Thursday, January 27, 2011 at 1:57am by Angela

Chemistry
Use the dilution relationship (Mi x Vi = Mf x Vf) to calculate the volume of 0.500 M NaOH needed to prepare 500 mL of .250 M NaOH. This is my work ? L Solution = 500mL x (1L/1000mL) = .500L ? mol NaOH = .500 L Solution x (0.250 M NaOH/1 L Solution) = .125 mol NaOH ? L solution...
Saturday, February 28, 2009 at 9:35pm by Bob

chemistry
A 20.0 mL sample of 0.687 M HBr is titrated with a 0.216 M NaOH solution. The pH after the addition of 10.0 mL of NaOH is __________. A. 0.413 B. 0.386 C. 0.163 D. 0.579 E. 0.237
Tuesday, July 24, 2012 at 10:44pm by katie

Science (Chemistry)
I'm not sure how to do a couple of problems on my chemistry worksheet. Can you please help me? You dissolve 0.00902 g of naOH in enough water to make 1000 mL. What is the Ph of this soultion. What is the molarity, pH, and pOH of 5.00 of naOH in 750.0 mL of soultion. I know how...
Sunday, November 6, 2011 at 10:18am by Dylan

Chemistry
What is the percentage strength (v/v) of Diluted Alcohol, NF, which results from mixing 50 mL of Alcohol, USP (95.0%, v/v) with 50 mL of Purified Water, USP? C1xV1 = C2xV2 95% x 50ml = C2 x 97ml C2 = 49% This was an example my professor put up. I can not comprehend why 97 ml ...
Monday, December 13, 2010 at 9:04pm by Anonymous

Physical chemistry 2
50 mL x 0.02M = 1 mmol HAc. 10 mL x 0.1M = 1 mmol NaOH. HAc + NaOH ==> H2O + NaAc 1 mmol 1mmol = e.p. So you have a solution of Ac^- in aqueous solution. The (Ac^-) is 1 mmol/60 mL = about 0.017M but you nee to do it more accurately. ........Ac^- + HOH ==> HAc + OH^- I...
Tuesday, March 12, 2013 at 12:41am by DrBob222

Chemistry
A sample of 25.00 mL of vinegar is titrated with a standard 1.02 M NaOH solution. It was found that a volume of 19.60 mL of the standard NaOH solution is used to completely neutralize the acetic acid in the solution. Calculate the concentration of the acetic acid solution.
Sunday, March 9, 2008 at 9:33pm by Allie

chemistry
millimoles NaOH = mL x M = 15 x 1.5 = 22.5 mmoles CH3COOH = 30 x 0.75 = 22.5 where CH3COOH = HAc. .........HAc + NaOH ==> NaAc + H2O initial..22.5...22.5.....0......0 change..-22.5..-22.5....+22.5..22.5 equil.....0......0.......22.5.... So you can see that the CH3COOH is ...
Tuesday, January 24, 2012 at 9:58pm by DrBob222

Chemistry
1. A good indicator will have a(n)____ close to this volume and pH. I think it's endpoint but it's wrong. 2. (part a) What is the pH of the solution created by combining 1.70 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)? ...
Saturday, April 28, 2012 at 3:38pm by Jody

Chemistry
Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below, followed by the pH of ...
Tuesday, May 27, 2008 at 7:38pm by Tom

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

Chemistry
A solution is made by mixing 37.0 mL of ethanol, C2H6O, and 63.0 mL of water.? Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? ethanol: 0.789 g/mL 43.9 torr water : 0.998 g/mL 17.5 torr
Saturday, March 2, 2013 at 1:05pm by Dee

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

chemistry
A buffer solution contains 0.200 M NH3 and 0.250 M NH4Cl. What is the pH of the buffer solution after the addition of 10.0 mL of 0.100 M NaOH to 50.0 mL of the buffer? Kb for NH3 is 1.8 x 10-5.
Tuesday, October 26, 2010 at 9:25pm by Brett

AP CHEMISTRY
1) Calculate the molarity of a solution of sodium hydroxide, NaOH,if 23.64 mL of this solution is needed to neutralize 0.5632g of potassium hydrogen phthalate. 2) It is found that 24.68 mL of 0.1165M NaOH is needed to titrate 0.2931 g of an unknown acid to the phenolphthalein ...
Thursday, March 8, 2012 at 6:27pm by HELP PLEASE

chemistry
a buffer is made by mixing 0.1 moles of acetic acd a sodium acetate in 500 ml of solution. determine the pH of the buffer. (Ka for acetic acid - 1.8E-5)
Wednesday, December 15, 2010 at 3:35pm by Tara

General Chemistry-Acids/Bases
I'm stuck on a couple of similar problems involving pH and acids/bases 1) What is the final pH of a 1L solution that is initially .15 M HF and .2 M NaF after 10 mL of .02 M HCl has been added? Ka=7.2x10^-4 Do i just calculate the total mols of H and divide by the volume, then ...
Wednesday, November 26, 2008 at 2:18pm by Evelyn

Chemistry
First write the equation and balance it. KOH + HOCl ==> KOCl + H2O moles HOCl = M x L = ?? To do these you simply need to figure out what you have in the solution, then apply the appropriate chemical properties and calculate. I will help you get started. The second thing ...
Saturday, April 17, 2010 at 11:30pm by DrBob222

Chemistry
A 50.0-mL sample of 0.10 M HNO2 is titrated with 0.10 M NaOH. What is the pH after 25.0 mL of NaOH have been added?
Tuesday, December 7, 2010 at 8:50pm by Eric

General Chemistry
millimoles HCl = 8.00 mL x 0.1M=0.8mmols. mmoles NaOH = 2.50 mL x 0.1M = 0.25 mmols. mmoles NaOH = 9.50 x 0.1M = 0.95 mmoles. mmoles HAc = 8.00 mL x 0.1M = 0.8 mmoles. -------------------------------------- ..........HCl + NaOH ==> H2O + NaCl initial...0.8....0........0...
Sunday, November 6, 2011 at 9:28pm by DrBob222

Chemistry -- to Dr.Bob
I had posted a while back and still couldn't solve this is there anyway you could show me the steps on how u did this? thank you very much A solution is made by mixing 20.0 mL of toluene C6H5CH3d=0.867gmL with 150.0 mL of benzene C6H6d=0.874gmL. Assuming that the volumes add ...
Saturday, April 5, 2008 at 8:05pm by Dora

Buffer Solution
You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH3COOH) and 0.20 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 93 mL of 1.00 M NaOH solution?
Wednesday, April 13, 2011 at 12:42am by Nicole

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 change...
Saturday, February 4, 2012 at 2:12pm 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

science:Chemistry
Find the pH of a solution obtained by mixing 100cm3 of 01MHCl solution with 100cm3 of 0.2M NaOH
Thursday, January 31, 2013 at 5:26pm by Anonymous

chemistry 101
If 15g of NaOh is dissolved in 285 g of water, calculate the following. Assume the density of the solution is 1.06 g/cc. a) Calculate the moles of NaOH in the solution? My answer is 15gNaOH/40g NaOH= .0375 mole NaOH b) Waht is the mass % w/w of the solution? My answer is 15g ...
Saturday, December 8, 2012 at 12:34am by Tracy

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

chemisry
A 0.1 molal solution of a weak monoprotic acid was found to depress the freezing point of water 0.1930C. Determine the Ka of the acid. You can assume 0.1 molal and 0.1 molar are equivalent. 100 ml of a 0.1M solution of the above acid is titrated with 0.1 M NaOH. After an ...
Sunday, February 12, 2012 at 3:16pm by ashley

Chemistry
Oh, thanks! That was so simple! I'm a little confused on how to set up this question? A solution is prepared by mixing 535 mL of 0.30 M NaOCl and 494 mL of 0.26 M HOCl. What is the pH of this solution? [Ka(HOCl) = 3.2 × 10-8] Could you give me a hint?
Monday, March 21, 2011 at 12:40am by Adrianna

Dr Bob
What is the pH of the solution that results from mixing 5 ml of 0.2 M NaOH and 100 mL of 0.05 M lactic acid? (Pka of lactic acid= 3.86) Responses Use the Henderson-Hasselbalch equation. The mixture you have indicated will react to form a buffer, the base will be the sodium ...
Sunday, January 11, 2009 at 7:15pm by Andrew

Chemistry
If 50.0mL of 1.60M HCl was added to 50.0mL of 1.80M NaOH, calculate the molarity of the resulting NaCl solution. (Hint: resulting solution has a volume of 100 mL)
Thursday, April 1, 2010 at 1:23am by Michelle

Chemistry
If 50.0mL of 1.60M HCl was added to 50.0mL of 1.80M NaOH, calculate the molarity of the resulting NaCl solution. (Hint: resulting solution has a volume of 100 mL)
Thursday, April 1, 2010 at 10:55am by Jen

chemistry help asap
Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample of NaOH solution is ...
Monday, February 6, 2012 at 8:20pm by missy

Chemistry105
When 50.0 Ml of 1.00 m chi was mixed with 50.0 ml of 1.00 m NaOH in a calorimeter the temperature rose from 25.0 c to 32.0 c calculate the heat change for the reaction assuming that the total volume of the solution is 100.0 ml and the specific heat is 1.00 cal/ (g.c). Is the ...
Sunday, December 2, 2012 at 7:16pm by Mira

Chemistry105
When 50.0 Ml of 1.00 m chi was mixed with 50.0 ml of 1.00 m NaOH in a calorimeter the temperature rose from 25.0 c to 32.0 c calculate the heat change for the reaction assuming that the total volume of the solution is 100.0 ml and the specific heat is 1.00 cal/ (g.c). Is the ...
Sunday, December 2, 2012 at 7:16pm by Mira

Chem
25.0 mL of 0.100 M acetic acid (Ka= 1.8 x 10^-5) is titrated with 0.100 M NaOH. Calculate the pH after the addtion of 27.00 mL of 0.100M NaOH. my work CH3COOH + H2O <-> H3O^+ + CH3COO^- 25mL x 0.100 mmol/ml = 2.5mmol CH3COOH 27mL x 0.100 mmol/ml = 2.7mmol NaOH There are ...
Tuesday, June 29, 2010 at 4:02pm by Anonymous

chemistry
a. A 0.1 molal solution of a weak monoprotic acid was found to depress the freezing point of water 0.1930C. Determine the Ka of the acid. You can assume 0.1 molal and 0.1 molar are equivalent. b. 100 ml of a 0.1M solution of the above acid is titrated with 0.1 M NaOH. After an...
Sunday, February 12, 2012 at 4:29pm by billy

Chemistry
Exactly 100 mL of 0.14 M nitrous acid (HNO2) are titrated with a 0.14 M NaOH solution. Calculate the pH for the following. (a) the initial solution (b) the point at which 80 mL of the base has been added (c) the equivalence point (d) the point at which 105 mL of the base has ...
Saturday, March 17, 2012 at 12:33am by Tanya

Chemistry
How many milliliters of 1.0 M NaOH must be added to 200. mL of 0.10 M NaH2PO4 to make a buffer solution with a pH of 7.50? (5 points)
Thursday, April 4, 2013 at 7:27pm by bill

chemistry
Consider the reaction HCl + NaOH ->NaCl + H2O Given: HCl Solution: 22 degrees celsius NaOH Solution: 22 degrees celsius Final Temperature: 26.1 degrees celsius A. Calculate the amount of heat evolved when 15 mL of 1.0 M HCl was mixed with 35 mL of 1.0 M NaOH B. Calculate ...
Monday, March 28, 2011 at 12:11pm by Vanessa

chem
a buffer is made by adding 150 ml of .595M BaF2 and 0f .500M of HF solution. calculate the pH of this buffer system calculate the pH of this buffer after adding .100 mol Hcl calculate the pH of this buffer after adding .0750 mol Ca(OH)2 ka(HF)= 6.9x10^-4 kb(F-)= 1.4 x 10^-11
Monday, March 1, 2010 at 11:37pm by simi

chemistry
I'm not sure you do. Do you mean something like, calculate the pH of 50 mL of 0.1 M HCl (pH = 1)when added to 50 mL H2O (neutral)? Or something different.
Wednesday, October 3, 2007 at 8:56pm by DrBob222

analytical chemistry
a 0.120 ml portion of a 50.0% (w/w) KOH solution having a density of 1.50*10^3 g/l is diluted to 250 ml. What is the pH of the resulting solution?
Saturday, March 30, 2013 at 10:50pm by lolo

Chemistry
Hello, I need help with calculations for lab. I prepared excess NaOH and HCL solutions (unknown conc., ~0.1M). Then I standardized my NaOH solution by titrating known amounts of KHP (Potassium hydrogen phthalate)with it in the presence of phenolphthalein (indicator turns pink ...
Sunday, September 20, 2009 at 2:05pm by Pavel

chemistry
A home swimming pool is disinfected by the daily addition of 0.50 gal (1 gal = 3.785 L) of a "chlorine" solution–NaOCl in NaOH(aq). To maintain the proper acidity in the pool, the NaOH(aq) in the "chlorine" solution must be neutralized. By experiment it is found that about 220...
Tuesday, October 9, 2012 at 6:08pm by joe

Chemistry
Part A: Unknown Acid use 1gram and mix with 120 mL of distilled water Determine the concentration of the acid by titrating with 0.0998 M of NaOH Concentration of NaOH= 0.0998M Volume of NaOH= 3.5 mL # moles of NaOH= Initial Concentration of Weak Acid- Show Calculation of Ka ...
Wednesday, March 24, 2010 at 3:40pm by Saira

Chemistry
A 25.0mL sample of a 0.100M solution of acetic acid is titrated with a 0.125M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added.
Monday, November 8, 2010 at 2:32pm by Amanda

Chemistry
One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concentration of NaOH is normally in the range of 3 to 6 M. The NaOH is analyzed periodically. In one such analysis, 45.7 ...
Wednesday, January 12, 2011 at 1:06am by Chin

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
This is a lab I have, but have no clue what to do. Please do out the steps so i can understand. Reactions and Data: NaOH(s)--> Na1+(aq)+ OH1-(aq) (Heat of solution of NaOH) This reaction involves adding solid NaOH to water and watching the temperature change as it dissolves...
Saturday, December 31, 2011 at 7:21pm by Carrie

analytical chemistry
What is the pH of a solution formed by mixing 14.35 mL of 0.200 F HCl with 0.322 g of Na3PO4, followed by dilution to 500.00 mL?
Tuesday, December 4, 2007 at 10:51am by Jonny

Chemistry
Predict whether or not a precipitate will form upon mixing 75.0 mL of a NaOH solution with pOH = 2.58 with 125.0 mL of a 0.018 M MgCl2 solution. Identify the precipitate, if any. Express as a chemical rxn NaOH(aq) + MgCl2(aq) => NaCl(s) + MgOH(aq) I have to balacnce it and ...
Sunday, October 31, 2010 at 3:34pm by Anonymous

chemisrty
A 21.00 sample of 0.3254M Hcl solution requires 26.09 ml of NaOH solution for complete neutralization. Calculate the volume of NaOH solution in liters, required for the titration.
Thursday, April 25, 2013 at 11:47am by ashley

Chemistry
Calculate the concentration, in molarity, of a solution prepared by adding 9 mL of water to 1 mL of 0.1 M HCl solution. If 2.0 mL of 0.010 M NaOH is mixed with enough water to make the total volume 8 mL, what is the molarity of the resulting solution?
Monday, October 3, 2011 at 6:09pm by Nico

Chemistry
1 g of acid was mixed with 120 ml of distilled water and the solution was filtered into a clean dry beaker. A 25 ml aliquot of this solution was titrated with 0.1120 M NaOH. The pH of the acid was recorded to be 4.42. Calculate the initial concentration of the weak acid and ...
Monday, March 25, 2013 at 6:12pm by Annie

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 1.00 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)? table 1: mL NaOH=1.00 ...
Tuesday, May 1, 2012 at 5:20pm by Heather

Chemistry
Consider the titration of 100.0 mL of 0.260 M propanoic acid (Ka = 1.3 ✕ 10−5) with 0.130 M NaOH. Calculate the pH of the resulting solution after each of the following volumes of NaOH has been added. (Assume that all solutions are at 25°C.) (a) 0.0 mL...
Sunday, December 8, 2013 at 1:31am by Rina

Chemistry
Convert 0.40 g NaOH to moles. Convert 50.0 mL x 0.1 M HCOOH to moles. See which is in excess. If NaOH, then calculate pOH and pH. If HCOOH, it will be a buffer and you should use the Henderson-Hasselbalch equation.
Wednesday, May 5, 2010 at 12:28pm by DrBob222

chemistry
Which solution would show the GREATEST change in pH on the addition of 10.0 mL of 1.0 M NaOH to 1.0 L of each of the following solutions? a. 0.50 M CH3COOH + 0.50 M NaCH3COO. b. 0.10 M CH3COOH + 0.10 M NaCH3COO. c. 0.50 M CH3COOH. d. 0.10 M CH3COOH. e. 0.50 M NaCH3COO. 4. (...
Thursday, May 13, 2010 at 5:27pm by wite2khin

chemistry
A chemist wishes to prepare 250mL of a buffer that is pH = 4.50. Beginning with 100mL of 0.12 mol L^(-1) acetic acid and a supply of 0.10 mol L^(-1) NaOH, explain how this could be done. How much 0.20 mol L^(-1) NaOH must be added to this buffer to raise the pH to 5.1? If the ...
Saturday, June 2, 2012 at 7:29pm by guess who

Chemistry Help! Thank you :)
Assuming the final solution will be diluted to 1.00 , how much more should you add to achieve the desired pH? Information: Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you: 100 ml of 7.00×10−2 M HCl, ...
Sunday, March 11, 2012 at 1:08am by Ashley

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