Wednesday
April 16, 2014

Search: calculate pH of KHP + NaOH

Number of results: 30,755

Chemistry
KHP + NaOH ==> NaKP + H2O So 1 mole KHP uses 1 mole NaOH. moles KHP = grams/molar mass. Calculate moles KHP Then moles NaOH = moles KHP M NaOH = moles NaOH/L NaOH. (mL NaOH used = final reading - initial reading, then convert to liters.)
Tuesday, October 4, 2011 at 8:50pm by DrBob222

Chemistry
got NaOH+KHC8H4O4-->H2O+KNaC8H4O4 is this correct? yes •Name the secondary standard used in the titration of the unknown KHP mixture. NaOH • Calculate the amount of NaOH (in millimoles) delivered in the titration. mL x M = millimols • Find the mass of KHP neutralized in the...
Wednesday, March 7, 2012 at 3:58pm by DrBob222

Chemistry
a. mol KHP = 0.4885g/molar mass = ? M = mols/0.1 L = approximately 0.024 but you need to do it more accurately. At the equivalence point the pH is determined by the hydrolysis of the P^2- ion. .........P^2- + HOH ==> HP^- + OH^- I.......0.024M...........0.......0 C...
Thursday, November 29, 2012 at 8:36pm by DrBob222

Chemistry
You probably intended this to be potassium hydrogen phthalate which I will rewrite, to make things simpler, as KHP. The H is the hydrogen neutralized by the NaOH. NaOH + KHP ==> NaKP + H2O. mols KHP = 1.029 grams/molar mass KHP. mols NaOH = mols KHP. mols NaOH = L x M. You ...
Thursday, November 1, 2007 at 9:20pm by DrBob222

Chemistry
You weighed KHP. Calculate the moles KHP you titrated with NaOH. Moles KHP = grams/molar mass. You should write the equation for KHP + NaOH but it is a 1:1 ratio (1 mole KHP to 1 mole NaOH). Therefore, moles KHP titrated will equal moles NaOH used. Then you know M x L = moles ...
Sunday, September 20, 2009 at 2:05pm by DrBob222

Chemistry
I don't know every step you followed; therefore, I'm hesitant to get into detail but here is what you should do. Make list on a page of each step you followed. Beside each step, place the calculation formula used for that step. Then analyze each step, take the results and go ...
Wednesday, March 7, 2012 at 9:47pm by DrBob222

chemistry
KHP is a monoprotic acid with a molar mass of 204.22 g/mol. The titration data are as following. The average concentration of NaOH solution is M. 1 2 3 mass of KHP (g) 2.789 2.543 2.612 vol NaOH used (mL) 27.77 23.22 27.12 You didn't ask a question but I assume you are to ...
Wednesday, May 16, 2007 at 1:41am by jared

chemistry
how do i calculate the NaOH molarity from a titration of KHP and NaOH after preparing KHP to standardise NaOH. KHP mass was 2.0378g dissoveld in distilled water to fill up a 100ml volumetric flask and only 10ml of this solution was used to in titration
Friday, March 22, 2013 at 7:00am by k

Chemistry
The equation is KHP + NaOH ==> H2O + KNaP moles NaOH = M x L = ?? Convert moles NaOH to moles KHP. That is 1:1 ratio (from the coefficients in the balanced equation) so moles KHP = moles NaOH. grams KHP = moles KHP x molar mass KHP %KHP = (grams KHP/0.847)*100 = ?? Note: ...
Sunday, July 31, 2011 at 11:24pm by DrBob222

chemistry
For the KHP question. Convert 0.51 g KHP to mols. mols = g/molar mass. You don't ask a question but I assume you want to know the molarity of the NaOH. Mols KHP = mols NaOH. mols NaOH = L x M. YOu have mols NaOH and L NaOH. Calculate molarity NaOH. Post yuor work if you get ...
Sunday, October 14, 2007 at 9:28pm by DrBob222

Chemistry
mols NaOH = M x L = ? mols KHP = same (1:1 ratio) from KHP + NaOH ==> KNaP + H2O. Calculate mass KHP from g = mols x molar mass. Then %KHP = (mass KHP/mass sample)*100 = ?
Wednesday, May 9, 2012 at 9:37am by DrBob222

Chem 2068 lab
No, you did it right but you labeled it wrong. moles KHP = 0.556 g KHP/204.33 = 0./00272 ( I wouldn't throw away the last 2). Then since 1 mole KHP = 1 mole NaOH, then M NaOH = moles NaOH/L NaOH = 0.00272/0.01448 = 0.1879 which to three significant figures rounds to 0.188 M. ...
Monday, October 18, 2010 at 9:12pm by DrBob222

Chemistry
0.01L KHP * 0.445M KHP = 0.00445 molKHP KHP and NaOH are in 1 to 1 ratio so, moles NaOH = 0.00445 so, 0.00445mol NaOH/ 0.01154L NaOH = 0.386M NaOH
Monday, October 4, 2010 at 7:30pm by Andrew

chemistry
I think the easiest way to work these "too small, too large, neither" problems is to go through the formula used to calculate the end result. I have summarized them here for problem #1. My comments are included with each in bold face. KHP standardization with NaOH. mols KHP = ...
Sunday, March 23, 2014 at 3:05pm by DrBob222

Chemistry
It would have been better to have typed in the numbers. As it is I don't know if you are right or not but it appears you are on the right track on parts and not on the right track for parts. mass KHP = (mass KHP + mass paper)-mass paper. volume NaOH = final buret reading - ...
Wednesday, October 26, 2011 at 10:55am by DrBob222

chem 111 lab
KHP + NaOH ==> NaKP + H2O mols KHP = grams/molar mass From the equation, mols KHP = mols NaOH. M NaOH = moles NaOH/L NaOH
Monday, February 20, 2012 at 6:22pm by DrBob222.

chemistry
NaOH + KHP ==> NaKP + H2O mols KHP = grams/molar mass mols NaOH = mols KHP (look at the coefficients in the balanced equation.) M NaOH = mols NaOH/L NaOH
Tuesday, December 11, 2012 at 3:57pm by DrBob222

chem 1
How much NaOH? Say 30 mL? moles NaOH = M x L = ? moles KHP = moles NaOH moles KHP = grams KHP/molar mass KHP. Solve for grams KHP
Monday, November 7, 2011 at 10:07pm by DrBob222

chemistry
KHP + NaOH ==> NaHP + H2O moles KHP = grams/molar mass Solve for moles. Look at the equation; it is 1:1 so moles KHP = moles NaOH.] The M NaOH = moles NaOH/L NaOH.
Saturday, October 16, 2010 at 12:26am by DrBob222

chemistry
I'll do the first one so you can see how it's done. First, write the formulas used to determine the molarity of the base. moles KHP = grams KHP/molar mass KHP moles KHP = moles NaOH. moles NaOH = mLNaOH x M NaOH and MNaOH = moles NaOH/mL NaOH. If the KHP is not dry, grams in ...
Sunday, April 18, 2010 at 2:19am by DrBob222

Chemistry
Most problems in chemistry hinge on mols. A mole reacts with one/two/three/etc mols of some other material. KHP + NaOH ==> NaKP + H2O mols NaOH = M x L = ? molsl KHP = mols NaOH (from the coefficients in the balanced equation). Then mols KHP = grams KHP/molar mass KHP. You ...
Saturday, December 1, 2012 at 9:16am by DrBob222

AP CHEMISTRY HELP
I think the best way to answer this type question is to write the steps involved in the procedure. Here is the KHP/NaOH problem. 1. mols KHP = grams/molar mass 2. mols NaOH = mols KHP 3. M NaOH = mols NaOH/L NaOH I presume not washing the paper on which the KHP was weighed ...
Thursday, December 20, 2012 at 9:05pm by DrBob222

chemistry
KHP + KOH ==> H2O + K2P. mols KHP = grams/molar mass mols NaOH = mols KHP (see coefficients in the balanced equation. M NaOH = mols NaOH/L NaOH
Wednesday, September 19, 2012 at 4:56pm by DrBob222

AP chemistry
moles KHP = grams/molar mass Substitute and solve for mols. KHP + NaOH ==> NaHP + H2O so the reaction is 1:1 and moles KHP = moles NaOH. Then M NaOH = moles NaOH/L NaOH. To obtain L NaOH, you will need to subtract the final buret reading - initial buret reading and convert ...
Sunday, October 24, 2010 at 8:29pm by DrBob222

Chemistry
So, Mols NaOH = 0.2264 M NaOH x 0.04936 L NaOH = 0.011175 Mols KHP = grams KHP / molar mass KHP or grams KHP = Mols KHP x molar mass KHP so 0.011175 x 204.22 = 2.2822 grams of KHP Is that correct DBob222?
Saturday, December 1, 2012 at 9:16am by T

Chemistry
I don't get 1.889 g KHP. mol NaOH = 0.01 x 0.1092 =0.001092 mols KHP = 0.0001092. mols KHP = grams KHP/molar mass KHP or g KHP = mols KHP x molar mass KHP = 0.0001092 x 204.22 = about 0.2230 g KHP.
Tuesday, October 9, 2012 at 3:08am by DrBob222

chemistry
calculate the mass of NaOH neded to prepare 500mL of a 0.10 M solution. I'm pretty sure the answer is 2g, but how do I get to that? Another question: calculate the molar amount of KHP used to neutralize the NaOH solution. .51 g of KHP was added to 50 mL of distilled H2O and a ...
Sunday, October 14, 2007 at 9:28pm by Rebecca

Chemistry(Please help, thank you!)
I shall be glad to check your results; however, you provided only the mass of the KHP. I need the volume of the NaOH solution used if you want the molarity of the NaoH. For the 1.00 g KHP, yes, moles KHP = 1.00/204.44 = ? but you did not do that correctly. It is 1.00g KPH x (1...
Monday, October 24, 2011 at 8:25pm by DrBob222

Help!!!!!!!!!!!!
A 0.391 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.
Monday, March 3, 2014 at 5:15pm by Jackie

Chemistry
A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP....? A student titrated 1.852 g of a mixture containing potassium hydrogen phthalate, KHP, with 0.163 M NaOH solution. She recorded an initial buret reading of 0.84 mL and a final buret ...
Wednesday, March 7, 2012 at 3:58pm by Cynthia

Inorganic chemistry
Potassium hydrogen phthalate (molar mass = 204.2g/mol) is used to standardize sodium hydroxide. If 26.37 mL of NaOH(aq) is required to titrate 0.7719g KHP to the equivalence point, what is the concentration of the NaOH(aq) (26.37 mL NaOH)(x) = (1 mol KHP/.7719g KHP)(204.2g KHP...
Tuesday, April 14, 2009 at 11:40am by Steve

Chemistry College
How much KHP is in samples 2 and 3? %KHP = (mL x M x mmolar mass/mass sample) You know mL NaOH, M NaOH, millimolar mass KHP is 0.20422; solve for %KHP. Then substitute %KHP and new mass of samples 2 and 3 and solve for mL NaOH.
Thursday, April 18, 2013 at 3:59am by DrBob222

Inorganic chemistry
mol KHP = (0.7719g)(1 mol KHP/204.2g) = .0038mol Where are the moles of NaOH? I know that there are 0.02637 L of NaOH and I know M = mol/l I know there are 40g NaOH/mol NaOH There is 1 mol of NaOH in the balanced equation But I do not have grams of NaOH
Tuesday, April 14, 2009 at 1:02pm by Steve

Chemistry
I think the % acetic acid will be too high. Standardization step: mols KHP = grams KHP/molar mass KHP mols NaOH = mols KHP M NaOH = mols NaOH/L NaOH Titration vinegar step: mols NaOH titrant = M x L mols acetic acid = mols NaOH g acetic acid = mols acetic acid x molar mass % ...
Friday, March 28, 2014 at 10:32pm by DrBob222

Analytical Chemistry
You have the mass of the KHP sample. You weighed out 0.5050 g (of course you've diluted it; perhaps that is the question; i.e., what is the mass of the KHP in the titrated sample? :-). How many moles NaOH did you use? M x L = moles = 0.0067M x 0.01475 = 9.88E-5 moles NaOH. ...
Wednesday, July 20, 2011 at 10:38am by DrBob222

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
I find it helpful to write each step of the procedure and see how the question affects each. 1. mols KHP = grams/molar mass 2. mols NaOH = mols KHP 3. M NaOH = mols NaOH/L NaOH So you did steps 1 and 2 right but on 3 added too much L NaOH. That's in the denominator, too big ...
Wednesday, December 5, 2012 at 3:17pm by DrBob222

Chemistry
NaOH + KHP ==> NaKP + H2O moles KHP = M x L = ?? moles NaOH = same (from the equation) M NaOH = moles NaOH/L NaOH
Monday, October 4, 2010 at 7:30pm by DrBob222

Chemistry
mool KHP = grams/molar mass mols NaOH = mols KHP (from the coefficients in the balanced equation.) M NaOH = mols NaOH/L NaOH
Thursday, October 17, 2013 at 5:13pm by DrBob222

chemistry
If the stockroom fails to dry the KHP to remove the waters of hydration, the student's calculated concentration for the standardized base will be: ____________ (low, high, or unaffected) A drop of NaOH is hanging from the buret tip before the titration of KHP. Once the student...
Wednesday, May 16, 2007 at 1:40am by jared

Chemistry
yes thank you i understand the parts for moles of KHP and NaOH. So the mw of KHP was given to me which was 204.44g/mol so for moles of KHP i did 1/204.44 and got 0.004 and then for NaOH i got 0.004 as well. Then for the concentration of NaOH would i do 0.004/0.0145 and 0.004/0...
Wednesday, October 26, 2011 at 10:55am by Hannah

Chemistry
From a titration of KHP and NaOH. Determine the range in NaOH volume to achieve a relative standard deviation of less than 0.2%. Assume 800mg of KHP was used.
Saturday, September 14, 2013 at 10:36pm by Mary

Chemistry
How does dissolved CO2 in distilled water affect the accuracy of the determination of a NaOH solution's concentration? How is the term acid anhydride applied here? I know you had answered this already, but what if KHP is used to titrate the NaOH. In this experiment KHP was ...
Saturday, March 29, 2014 at 9:38pm by Sandy

chemistry
mols KHP = grams/molar mass You took 10mL from 100 so you took 1/10 of those mols to titrate. Then mols NaOH = same as mols in the titrated KHP. M NaOH = mols NaoH/L NaOH.
Friday, March 22, 2013 at 7:00am by DrBob222

Chemistry
KHP or potassium hydrogen phthalate is a monoprotic acid used as a primary standard. so KHP + NaOH -> KNaP + H2O if 0.1803 g of KHP has been used, this is 0.1803 g/204.2 g mol^-1 =8.829 x 10^-1 mole which reacts with the same number of moles of NaOH so concentration of NaOH...
Thursday, December 9, 2010 at 8:51am by Dr Russ

Chemistry
A Student Performing a lab weighed a 1.0993g sample, containing an unknown KHP, which required 18.06mL of 0.1879M NAOH to reach the phenolphtalein endpoint. a) How many moles of base were consumed by the KHP in this sample? b) How many grams of KHP were titrated? c)What is the...
Wednesday, May 9, 2012 at 9:37am by Brittany

Chemistry
Write the equation and balance it. Convert 1.8 g KHP to moles. moles = grams/molar mass Convert moles KHP to moles NaOH using the coefficients in the balanced equation. Finally, M NaOH = moles NaOH/L NaOH. Solve for L NaOH and convert to mL.
Sunday, October 9, 2011 at 10:24pm by DrBob222

Chem 2068 lab
I wonder if you REALLY have the molarity of KHP. Usually that is a solid and one weighs it as a solid and titrates the entire sample; thus, moles is the number we needed. However, if you mean what you say, then mL x M = mL x M. Since you don't list a volume for KHP, I suspect ...
Monday, October 18, 2010 at 9:12pm by DrBob222

Chem
moles KHP = grams/molar mass. moles NaOH = moles KHP (write the equation to see that it is a 1:1 ratio). M NaOH = moles NaOH/L. Yo will need to subtract the final buret reading from the initial buret reading to obtain the total mL NaOH used, then convert to L to substitute ...
Tuesday, July 13, 2010 at 5:09pm by DrBob222

Chemistry
yes. Write the equation and look at the coefficients. KHP + NaOH ==> NaKP + H2O 1 mol KHP = 1 mol NaOH
Thursday, October 17, 2013 at 5:13pm by DrBob222

Chemistry
For a chemistry lab the experiment was to carry out an acid-base titration to determine the exact concentration of a sodium hydroxide solution. Two trials were completed and the data collected was: mass of weighing paper, mass of weighing paper + KHP, mass of KHP, initial ...
Sunday, October 23, 2011 at 3:30pm by Hannah

chemistry
The KHP used in the titration with NaOH was contaminated with sodium hydrogen phyhalate (NaHC8H4O4), but you didn't know it. State the effect of the final result (falsely high, falsely low, or unaffected) Explain. thanks These problems must be reasoned through. (1)mols KHP = ...
Wednesday, September 20, 2006 at 1:38pm by bria

Chem 2068 lab
Did i get it wrong? It has KHP molar mass at 204.33 g/mol and we use 0.556 g of KHP dissolved in water. THen if 14.48 mL of NaOH is used to reach endpoint, it needs the concentration of NaOH?
Monday, October 18, 2010 at 9:12pm by Car

Inorganic chemistry
Okay, mol KHP = (0.7719)(mol KHP/204.2g KHP) = .0038mol Since this is a titration then the moles of NaOH = the moles of KHP M = mol/L M = .0038mol/02637 M = 0.01441
Tuesday, April 14, 2009 at 2:52pm by Steve

Chemistry
moles KHP = grams/molar mass moles NaOH = moles KHP M NaOH = moles NaOH/L NaOH
Sunday, October 23, 2011 at 3:30pm by DrBob222

Chem
mols KHP = grams/molar mass = ? mols NaOH = mols KHP M NaOH = mols NaOH/L NaOH.
Tuesday, October 9, 2012 at 3:09am by DrBob222

Chemistry
mols KHP = grams/molar mass mols NaOH = mols KHP M NaOH = mols NaOH/L NaOH
Tuesday, October 16, 2012 at 5:31am by DrBob222

Chem.
mols KHP = grams/molar mass = ? mols NaOH = mols KHP M NaOH = mols NaOH/L NaOH
Monday, March 17, 2014 at 3:02pm by DrBob222

Chemistry
For a chemistry lab the experiment was to carry out an acid-base titration to determine the exact concentration of a sodium hydroxide solution. Two trials were completed and the data collected was: mass of weighing paper, mass of weighing paper + KHP, mass of KHP, initial ...
Wednesday, October 26, 2011 at 10:55am by Hannah

Chemistry(Please help!!)
For a chemistry lab the experiment was to carry out an acid-base titration to determine the exact concentration of a sodium hydroxide solution. Two trials were completed and the data collected was: mass of weighing paper, mass of weighing paper + KHP, mass of KHP, initial ...
Sunday, October 23, 2011 at 6:19pm by Hannah

Chem.
To standardize a solution of NaOH, one uses a primary standard called potassium hydrogen phthalate (KHP). It is a monoprotic acid. It has a molar mass of 204.33g/mol. Suppose you weigh out .556g of KHP and dissolve it in water. It requires 14.48 mL of NaOH to reach the ...
Monday, March 17, 2014 at 3:02pm by Anonymous!

chemistry...
knowing that one mole of KHP, C8H5O4K, reacts with one mole of NaOH, what mass of KHP is required to neutralized 30.0mL of the 0.10 M NaOH solution?
Tuesday, October 23, 2012 at 3:44pm by tierra

AP CHEM
Hello, I'm working these homework questions out; however it is a series of questions and without one step correctly completed, it's nearly impossible to get the others. I posted my work and commented where I need assistance. Thank you so much in advance!!! Potassium hydrogen ...
Thursday, April 17, 2008 at 8:31pm by Sigurd

general chemistry
First, determine the approximate number of grams of KHP. moles = M x L = 0.1005M x 0.020 L = ?? moles NaOH. moles KHP = moles NaOH. grams KHP = moles KHP x molar mass KHP = xx grams KHP. %KHP = (grams KHP/mass sample)*100 = 50 You know grams from the calculations above, ...
Sunday, October 17, 2010 at 11:21am by DrBob222

chemistry
You don't have questions here. Mostly just statements. Here is the equation. HA + NaOH ==> H2O + NaA I assume the benzoic acid was titrated with the NaOH and the question is to determine the molar mass of benzoic acid. LNaOH x M NaOH (from part a) = moles NaOH. moles HA = ...
Friday, November 4, 2011 at 1:19am by DrBob222

chemistry
HCL is tritrated with NaOH. KHP is then added. A possible source of systematic error in this experiment is failure to dry the KHP. If this occured, would the final wt% NA2CO3 be falsely high, falsely low, or unaffected. Give reasoning. Thanks. You have left out much of the ...
Wednesday, September 6, 2006 at 2:02pm by bria

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

AP CHEM
Potassium hydrogen phthalate is a weak solid acide w/ the formula KHc8H4O4 (often abbrv. KHP) and a formula weight of 204.23 g/ mole. It is often used to standardize a solution of a strong acid with an unknown concentration(Actually KHP is used to standardize a base and that ...
Thursday, April 17, 2008 at 8:31pm by DrBob222

chemistry
Ratio of what NaOH to mass KHP. You want the mass ratio? mass NaOH = M x L and grams NaOH = mols NaOH x molar mass NaOH. Then mass ratio is mass NaOH:mass KHP.
Wednesday, January 9, 2013 at 12:28am by DrBob222

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(Please help, thank you!)
For a chemistry lab the experiment was to carry out an acid-base titration to determine the exact concentration of a sodium hydroxide solution. Two trials were completed and the data collected was: mass of weighing paper, mass of weighing paper + KHP, mass of KHP, initial ...
Monday, October 24, 2011 at 8:25pm by Hannah

Chemistry
When 50.0ml of 1.00M HCl is titrated with 1.00M NaOH, the pH increases. calculate the difference in pH of the system when you add 49.99ml NaOH and 50.01ml of NaOH. Please work out detailed steps.
Friday, March 29, 2013 at 2:47pm by Grace

College Chemistry
You can do one or two things for that cubed symbol. You can write cm^3 (the caret means raised to the power in computer language), OR you can write the volume as cc. 36.78 cm^3 = 38.78 cubic centimeters = 38.78 cc. A cc = mL also. mols KHP = grams/molar mass = ?? moles NaOH = ...
Friday, October 22, 2010 at 12:05am by DrBob222

Chemistry
Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic acid=4.75) I got pH= 3.88 ...
Sunday, February 27, 2011 at 12:49pm by Jon

Chemistry
Look at how you calculated the M of the NaOH. You had KHP and moles= grams/molar mass. Then M NaOH = moles/L So if some of the KHP was spilled, that means grams was too low, which makes moles too low and if moles is too low when plugged into M NaOH, then moles/L will be too ...
Tuesday, March 3, 2009 at 12:12am 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
The question gives you the pH and asks you to calculate the concentration of the hydroxide ion. (OH^-) is read as "the concentration of the hydroxide ion". Actually it is NaOH which the problem uses but since the NaOH is 100% ionized in solution, then (NaOH) and (OH^-) are the...
Wednesday, May 7, 2008 at 9:35pm by DrBob222

chemistry
Calculate the pH of the following solutions. (A) 0.95 NaOH (B) 9.9x10^-10 M NaOH (C) 6.7 M NaOH
Saturday, May 4, 2013 at 2:02pm by wes

Chemistry
Hi everyone, I have been trying to figure out this titration equation all day and for some reason I am stumped. Here is the question in full: Potassium hydrogen phthalate, KHP, can be obtained in high purity and is used to determine the concentrations of solutions of strong ...
Thursday, November 29, 2012 at 8:36pm by jo

chem
You need to know the molarity of the NaOH. The 204.2 sounds like you standardized the NaOH by using 0.4321 g of pure potassium hydrogen phthalate. moles KHP = 0.4321/204.22 = ? moles NaOH = moles KHP M NaOH = moles NaOH/0.02435 You can work out the M NaOH. Now all we need to ...
Monday, February 13, 2012 at 10:06am by DrBob222

AP Chemistry
moles KHP = grams/molar mass You are titrating one H with one OH; therefore, moles NaOH must be the same as moles KHP. moles NaOH = M x L. YOu know moles NaOH and volume (in mL, convert to L and volume = difference in final buret reading - initial buret reading). Solve for M
Wednesday, September 14, 2011 at 9:26pm by DrBob222

Chemsitry
Calculate the weight of KHP that will react with 25mL of .1M NaOH
Tuesday, October 19, 2010 at 4:07pm by Sierra

chemistry
A 50.00ml sample of 0.200M hydroflouric acid (HF) is titrated with 0.200M NaOH. The Pka of HF is 3.452. a) calculate the pH of the HF solution before titration b) calculate the pH after the addition of 20.00ml of NaOH
Saturday, November 6, 2010 at 5:04pm by michelle

chemistry
HCl + NaOH ==> NaCl + H2O At zero mL. YOu have 0.1 M HCl so the pH is pH = -log(H^+). Since HCl is a strong acid, H^+ = 0.1 M and pH = 1. All of the others are done this way: a. moles HCl initially = M x L = 0.025 x 0.1 = 0.0025 moles HCl. b. moles NaOH added. (at 5 mL this...
Friday, April 30, 2010 at 12:08pm by DrBob222

chemistry
mols KHP = grams/molar mass M base = mols KHP/L base. If the KHP is wet, the mass of the KHP weighed will be too low (because some of the mass is water). of grams is too low in equation 1, then mols is too low. If mols is too low in equation 2, then M base is too low. Assuming...
Tuesday, April 1, 2008 at 2:27pm by DrBob222

Chemistry help
NaOH is a strong base, so it will completely dissociate into OH-. pOH+pH=14, so 14-pOH=pH Solve for pOH 2.00g of NaOH*(1 mole of NaOH/39.997 g)= moles of NaOH moles of NaOH/2.00L=molarity of NaOH -log[molarity of NaOH]=pOH 14-pOH=pH
Monday, July 29, 2013 at 7:36pm by Devron

Biochemistry DR.BOB
Isn't a phosphate buffer @ pH about 7.2 composed of NaH2PO4 and Na2HPO4? So you must add enough NaOH to completely neutralize the first hydrogen; therefore, you add 100mL x 0.1M mmoles NaOH to START. Then calculate the base(HPO4--/H2PO4-) you need to ADD to the NaOH initially ...
Tuesday, February 1, 2011 at 5:30pm by DrBob222

CHEMISTRY
Not for homework, just practice problems I'm having trouble with. Knowing that one mole of KHP, C8H5O4K, reacts with one mole of NaOH, what mass of KHP is required to neutralize 30.0 mL of the 0.10 M NaOH solution? if 24.5 mL of the 0.10 M NaOH solution is required to reach ...
Monday, October 22, 2012 at 8:20pm by Kimberly

Analytical Chemistry
How do I find the mass of KHP? 0.5050 grams of KHP was used and placed into a 250mL volumetric flask and diluted to the mark with distilled water. 50.00mL of this KHP solution was placed in a 250mL beaker. It took 14.75mL of 0.0067M of NaOH to reach the endpoint. What is the ...
Wednesday, July 20, 2011 at 10:38am by Linda

chemistry
i have to find the ratio of naoh:mass of KHP. but i have volume oh NaOH and mass of KHP and i dont know how to find the ratio then plz help me right now.
Wednesday, January 9, 2013 at 12:28am by Riana

chemistry
Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. If the impurity is neither acidic or basic, ...
Tuesday, March 11, 2014 at 2:25am by Sandy

CHEMISTRY PLEASE HELP
a)Here are the equations used for the standardization of NaoH> 1. moles KHP = grams/molar mass 2. moles NaOH = moles KHP 3. M NaOH = moles NaOH/L NaOH If KHP is spilled that means grams is too small in equn 1 which makes moles small; eqn 2 makes moles NaOH too small, #3 ...
Monday, October 24, 2011 at 8:03pm by DrBob222

Chemistry, pH, Buffers
Please help!! 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 me how do I calculate the Ka of the unknown acid and the ...
Monday, April 2, 2012 at 11:44am by Krina

chemistry
Look at the equation. Base + acid = salt + water. NaOH + HC2H3O2 ==> NaC2H3O2 + H2O Calculate the moles NaOH to start. Calculate the moles HC2H3O2 to start. I haven't done the calculation but I assume that the HC2H3O2 will be in excess and all of the NaOH will be used. So ...
Monday, July 13, 2009 at 7:29pm by DrBob222

Chemistry
Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. If the impurity is neither acidic or basic, ...
Friday, March 28, 2014 at 10:32pm by Sandy

general chemistry
A student needs to determine by titration with NaOH the precise %KHP in an unknown sample that is thought to contain approximately 50%KHP. Approximately what mass of sample should the student use in order to use about 20mL of 0.1005 M NaOH to reach the endpoint of the ...
Sunday, October 17, 2010 at 11:21am by Rosie

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

College Chemistry
A student weighs out 0.568 g of KHP (molar mass=204g/mol) and titrates to the equivalence point with (36.78 cm cubed which is 3) of a stock NaOH solution. What is concentration of stock NaOH solution? KHP is an acid with one acidic proton. The word cubed is in word form ...
Friday, October 22, 2010 at 12:05am by Elleni

Chem
a solution of sodium hydroxide is standardized against potassium hydrogen phthalate (KHP, formula weight 204.2 g/mol). From the following data, calculate the molarity of the NaOH solution: mass of KHP 1.054 g; buret reading before tiltration 0.33 mL; buret reading after ...
Tuesday, July 13, 2010 at 5:09pm by debbie

CHEMISTRY
a solution of sodium hydroxide is standardized against potassium hydrogen phthalate (KHP, formula weight 204.2 g/mol). From the following data, calculate the molarity of the NaOH solution: mass of KHP 1.404 g; buret reading before titration 0.13 mL; buret reading after ...
Friday, October 18, 2013 at 7:32pm by maria

Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>

Search
Members