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August 29, 2014

Search: calculate pH of KHP + NaOH

Number of results: 20,013

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 ...
May 16, 2007 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
March 22, 2013 by k

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...
April 14, 2009 by Steve

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 ...
October 14, 2007 by Rebecca

science-chemistry
We performed a titration with NaOH solution with KHP. Now I need to calculate the average molarity of NaOH based on this data Weight of khp= 0.1083 g Volume of naoh = 6.4 ml Then if i get this how do i get the molarity of ch3cooh totrated in naoh with the data Volume of ...
April 23, 2014 by cassy

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 ...
March 7, 2012 by Cynthia

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.
March 3, 2014 by Jackie

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
April 14, 2009 by Steve

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...
May 16, 2007 by jared

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...
May 9, 2012 by Brittany

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.
September 14, 2013 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 ...
March 29, 2014 by Sandy

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 ...
October 26, 2011 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 = ...
September 20, 2006 by bria

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 ...
October 23, 2011 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 ...
March 17, 2014 by Anonymous!

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 ...
October 23, 2011 by Hannah

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
April 14, 2009 by Steve

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 ...
September 6, 2006 by bria

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 ...
October 24, 2011 by Hannah

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?
October 23, 2012 by tierra

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 ...
October 22, 2012 by Kimberly

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 ...
April 17, 2008 by Sigurd

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 ...
July 20, 2011 by Linda

Chemsitry
Calculate the weight of KHP that will react with 25mL of .1M NaOH
October 19, 2010 by Sierra

Chem Question
What is the molarity of a NCL solution if 37.50 mL of the acid is needed to neutralize 25.00 mL of 0.0725 M NaOH? I'm not quite sure how to go about doing this one. And also this one thing. The following technical errors were committed in standardizing the NaOH. What will be ...
March 8, 2007 by Angie

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 ...
July 13, 2010 by debbie

AP 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 1.234 g; buret reading before titration 0.23 mL; buret reading after ...
September 14, 2011 by Chandler

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 ...
October 18, 2013 by maria

AP chemistry
A solution of sodium hydroxide is standard- ized 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 1.894 g; buret reading before titration 0.13 mL; buret reading after ...
October 24, 2010 by Anonymous

Chemistry
A solution of sodium hydroxide is standard- ized 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 1.654 g; buret reading before titration 0.23 mL; buret reading after ...
October 4, 2011 by Broy

chemistry
A solution of sodium hydroxide is standard- ized 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 1.744 g; buret reading before titration 0.13 mL; buret reading after ...
September 19, 2012 by cheri

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 ...
October 22, 2010 by Elleni

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, ...
March 11, 2014 by Sandy

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, ...
March 28, 2014 by Sandy

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.
January 9, 2013 by Riana

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 ...
October 17, 2010 by Rosie

Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
October 20, 2010 by James

College Chemistry
"A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated cylinder to obtain ...
October 20, 2010 by James

College Chemistry
The Question Is: "A student weighs 0.347 g of KHP on a laboratory balance. The KHP was titrated with NaOH and the concentration of the NaOH determined to be 0.110 M. For the second titration, the student correctly diluted 6 M HCl from the reagent shelf using a graduated ...
October 19, 2010 by James

Chemistry College
If KHP sample 1 requires 22.47 mL of aqueous NaOH, how many milliliters of NaOH should be needed for samples 2 and 3?
April 18, 2013 by Belinda

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 ...
September 20, 2009 by Pavel

Chemistry
How to find the molarity of NaOH when the given is 0.1803 grams of KHPg/mol molecular w. of KHP is 204.2 9.7 ml NaOH
December 9, 2010 by prince

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 ...
November 29, 2012 by jo

College Chemistry
I need help with this question!! a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid was first dissolved in...
April 25, 2012 by Emily

chemistry
Determine the mass of KHP (molar mas = 204.2 g/mol) that is required to react with 30.0 mL of 1.0 M Na0H (molar mass 40.0 g/mol)if the reaction is NaOH + KHP --> NaKP + H2O
October 13, 2011 by chris

chemistry
If the 12.5ml of NaOH solution is required to react completely with 0.300g of KHP (Potassium Hydrogen Phthalate, 204.2g/mol). What is the molarity of NaOH?
December 11, 2012 by paul

Chemistry
Calculate the grams of KHP needed to react with 25.2 ml of 0.10M KOH if the reaction is? KOH+KHP -----> K2P + H2O
October 3, 2011 by Dante

Chem
A 0.2181 g sample of KHP required 17.29 mL of sodium hydroxide solution to reach the phenolphthalein end point. Calculate the molarity(M) of the NaOH solution.
October 9, 2012 by Donnie

Chem 2068 lab
Once I have the molarity for KHP which is 0.0027 M, and i add 14.48 mL of NaOH to the solution, what is the concentration of NaOH in the solution.
October 18, 2010 by Car

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 begins the ...
April 1, 2008 by Confused

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 begins the ...
April 18, 2010 by help

chem 1
a NaOh solution has a concentration of about 0.11M.How many grams of KHP would have to be used to require NaOH solution to reach the endpoint
November 7, 2011 by karen

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 ...
December 8, 2012 by Tracy

Chm General 2
if a student doing an experiment failed to dry the KHP before using it to standarize the NaOH solution. A) Would her calculated molarity of the NaOH solution probably be too hight or too Low?
March 23, 2011 by Karla

Inorganic chemistry
Potassium hydrogen phthalate (molar mass = 204.2 g/mol is used to standardize sodium hydroxide. If 23.67 ml of NaOH (aq) is required to titrate 0.7719 g KHP to the equivalence point, what is the concentration of the NaOH(aq)? HC8H4O4-(aq) + OH-(aq) = C8H4O4^2-(aq) + H2O(l)
April 11, 2009 by Steve

chemistry
Mass of "KHP" to neutralize 18 mL of 0.20 M NaOH?
February 25, 2011 by sallay

chemistry
2. When preparing a NaOH solution, a student did not allow the NaOH pellets to completely dissolve before standardizing the solution with KHP. However, by the time the student refilled the buret with NaOH to titrate the acetic acid, the remaining NaOH pellets had ...
March 24, 2014 by anonymous

Chemistry
What mass (g) of KHP is required to neutralize 10.00 mL of 0.1092 M NaOH?
October 9, 2012 by Erin

chem 111 lab
if a student used 12.45mL of their NaOH solution to neutralize 10.00mL of a 0.543 KHP solution, then what is the concentration of the student's NaOH solution?
February 20, 2012 by danielle

Chemistry
If a student used 11.54mL of their NaOH solution to neutralize 10.00mL of a 0.445M KHP solution, then what is the concentration of the student's NaOH solution (in Molarity)?
October 4, 2010 by Ari

Chemistry - Molarity
Potassium hydrogen phthalate is a monoprotic acid. Dihydrogen phthalate (H2C8H4O4) is a diprotic acid. An analyte sample contains 0.127 M KHP and 0.0678 M H2C8H4O4. What volume of a 0.205 M NaOH solution is required to neutralize 25.0 mL of the analyte solution? Molar masses: ...
December 10, 2012 by Amy

Chemistry
A sample of 1.018 g of KHP (potassium hydrogen phthalate, molar mass = 204.22 g/mol) was dissolved in ~ 25 mL distilled water and titrated with a NaOH solution of unknown concentration. If 28.69 mL of base was used to reach the endpoint, what was the concentration of the NaOH...
October 17, 2013 by Maya

Burnett
Write balanced molecular and net ionic equations for the reaction of KHP with NaOH.
October 9, 2011 by Mariah

General Chemistry
Starting out with 50 mL of 0.20 M NaHCO3, calculate how many mL of 0.50 M NaOH solution to add to make 100 mL of approximately 0.10 M (total) buffer solution with a pH of 10.35. By adding NaOH, some of the NaHCO3 gets converted to the conjugate Na2CO3. This conjugate acid/base...
April 3, 2012 by Lucy

Chemistry
How many mL of the 0.1029 M standard NaOH solution is required to titrate 0.2247 g sample of KHP to the phenolphthalein end point?
October 9, 2012 by Erin

college chemistry
If KHP sample #1 requires 27.30 mL of NaOH solution to reach an endpoint, what volume should be required for samples #2 and #3?
October 25, 2012 by Kristen

chemistry
1. When performing this experiment, a student mistakenly used impure KHP to standardize the NaOH solution. If the impurity is neither acidic nor basic, will the percent by mass of acetic acid in the vinegar solution determined by the student be too high or too low? Justify ...
March 23, 2014 by anonymous

chemistry
When filling the buret with NaOH solution, you left an air bubble in the buret tip. The bubble was released durning your first KHP titration. Would the following technique error result in an erroneously high or reeoneously low calculated molarity of NaOH solution? explain ...
February 22, 2010 by Diane

Chemistry
In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student refilled the buret with NaOH to titrate ...
March 29, 2014 by Sandy

College Chemistry
1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample of an unknown monoprotic acid is titrated with...
October 25, 2010 by Jessica

Math
1. Write the balanced chemical equation for the reaction NaOH + HCI --> NaCI + H20 2. Extract the relevant information from the qustion: NaOH v= 30mL, M=0.10 HCI v= 25.0 mL, M=? 3. Convert to Liters NaOH v= 0.03 L, M= 0.10M HCI v=0.025L, M=? 4. Calculate moles NaOh: n(NaOH...
March 8, 2010 by Maria

Chemistry help
I am confused as to how to solve the below problem. I am not sure which formula to use. At first I thought I calculate the molar mass of NaOH, followed by calculating moles of NaOH. But I don't have the mass of NaOH to calculate moles. Do I convert 10mL to grams to Be able to ...
March 15, 2012 by Julie

Chemistry
A student actually used 0.847g sample of impure KHP and the endpoint was reached after 19.82 ml of sodium hydroxide solution was added, What is the percent KHP in the unknown to four significant figures.
July 31, 2011 by BEE

Chemistry
A student actually used 0.847g sample of impure KHP and the endpoint was reached after 19.82 ml of sodium hydroxide solution was added, What is the percent KHP in the unknown to four significant figures.
August 1, 2011 by BEE

Chemistry
How many grams of KHP (204.22 g/mol) were present in container if 49.36 mL of 0.2264M NaOH were needed to reach the end point of a titration? I'm confused on the formula you would use for this.
December 1, 2012 by T

Chemistry (heat flow, simple)
Well I know to calculate heat flow you use, q=ms delta t. for this experiment we mixed naoh with hcl into water. the total mass (volume) of the mixture was 100g the temperature change for naoh was 11.7 degrees C and for hcl it was 11.8 degrees C now im looking to calculate ...
March 12, 2010 by Abdullah

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

chemistry
Can you help me with the following: Calculate hte pH that results when 25 mL of .1M HCL is titrated with .1M NaOH solution run in from a buret at each of the stages of volume of .1 M NaOH add in 5.0 mL incrememnts beginning with 0 mL of NaOH
April 30, 2010 by Cathy

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) ...
April 21, 2013 by LUx

chemistry
a student dissolves 0.625 g of pure benzoic acid in distilled water and titrated the resulting solution to the equivalence point using 40.8 mL of the standardized NaOH solution from Part a, assuming that benzoic acid has only one ionizable hydrogen, answer the following: ...
November 4, 2011 by Anonymous

Chemistry
A 0.355 g sample of a solid, monoprotic acid having a molar mass of 121 g/mol requires 18.47 mL NaOH for neutralization. Calculate the molarity of the NaOH solution. I got 0.159 M NaOH
July 11, 2013 by <3

AP CHEM
Please help me with thses AP CHEM homework problems and show the steps to how to find the solutions: Solid Liquid Titrations: Determine the concentration of the indicated liquid unknown given the mass of a solid standard and the buret data for the titration. #35) What is the ...
July 31, 2008 by shylo

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...
February 28, 2009 by Bob

Chemistry
A student dissolved the KHP in 100.0mL of water instead of 50.0mL. Will the molar concentration of the NaOH solution determined from titrating be greater, less than, or unaffected by this mistake? Explain.
April 2, 2013 by Lola

Chemistry
A titration involves titrating 0.4 M NaOH into a solution of 0.2 M H3PO4. a.) Calculate the volume of NaOH that will be required to reach the first equivalence point. b.) Calculate the volume of NaOH required to reach the second equivalence point. Other information: 10 ml ...
February 8, 2014 by Anonymous

Chemistry
In this case, the inflection point, and equivalence, occurs after 23.25mL of 0.40 M NaOH has been delivered. Moles of base at the equivalence point can be determined from the volume of base delivered to reach the equivalence point and the concentration of NaOH. 1. Calculate ...
October 21, 2010 by John

math
50gm of a sample of ca(oh)s is dissolved in 50ml of 0.5N hcl solution. The excess of hcl was titrated with 0.3N -naoh. The volume of naoh used was 20cc. Calculate of naoh used was 20cc. Calculate % purity ca(oh)2 Who help me step by step
December 22, 2013 by Fai

Chemistry
a 15.00mL sample of NaOH was titrated to the stoichiometric point with 17.40mL of 0.2340M HCl. a) what is the molar concentration of the NaOH solution? b)calculate the grams of NaOH in the solution.
December 9, 2010 by prince

Grade 12 chemistry
This is the second reaction: HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l) (Heat of neutralization) This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl. Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL of the HCl. The temperature rises from 22.00...
January 1, 2012 by tessa

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...
December 31, 2011 by Carrie

chemistry
Calculate the amount of NaOH in this solution 5.00mL of 12.0 NaOH is diluted with water to make 24 mL of 2.50 NaOH solution
April 24, 2012 by crystal

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.
March 29, 2013 by Grace

Chemisty
Calculate the number of milliliters of 0.738 M NaOH required to precipitate all of the Mg2+ ions in 148 mL of 0.541 M MgSO4 solution as Mg(OH)2. The equation for the reaction is: MgSO4(aq) + 2 NaOH(aq) Mg(OH)2(s) + Na2SO4(aq) _____________mL NaOH
February 7, 2012 by Eliazbeth

Chemistry
A 50.0 mL sample of 0.12 M formic acid, HCOOH, a weak monoprotic acid, is titrated with 0.12 M NaOH. Calculate the pH at the following points in the titration. Ka of HCOOH = 1.8 multiplied by 10-4. What is the pH when 50.0 mL NaOH is added 60.0 mL NaOH is added 70.0 mL NaOH is...
April 3, 2011 by George

chemistry
If it requires 30.0 milliliters of 1.2 molar HCl to neutralize 20.0 milliliters of NaOH, what is the concentration of the NaOH solution? Balanced equation: NaOH + HCl NaCl + H2O 0.60 M NaOH 0.80 M NaOH 1.3 M NaOH 1.8 M NaOH
June 22, 2011 by Magan

Chemistry
Hi, I posted yesterday with this lab question. "Calculate the molar amounts of NaOH used in the reaction with the HCl solution and with the HC2H3O2. I think I got the answer to that with the help that I received. I had 5 mL of HCl, and I was using .100 M NaOH, so I got 5x10-4 ...
April 22, 2007 by Rachel

chemistry
In experiment concerning potentiometric determination of puriy and Ka of KHP, we obtained an experimental pKa of 5.04 and when compared with the theoretical pKa of 5.51, we obtained a % relative error of 192%. Could this error mean that a cerain impurity in the KHP sample ...
September 10, 2007 by smiley

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 ...
March 28, 2011 by Vanessa

Chemistry II
Calculate the change in heat: 2 Na(s) + 2 H2O(l) > 2 NaOH(aq) + H2(g) So far this is what I have: 2 H20 --> 2 H2 + O2 2(285.83) kJ 2 Na + O2 + H2 --> 2 NaOH 2(-426.73) kJ 2 Na + 2 H2O --> 2 NaOH + H2 -281.8 kJ If this correct?? yes, correct, as best as I can tell.
May 20, 2007 by Jayd

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