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October 25, 2014

Search: chem-acid base titrations

Number of results: 17,377

Chemistry
We did a lab for acid-base titrations, and I'm having trouble with my post lab questions because I had trouble with acid-base reactions and titrations in the first place! "Calculate the molar amounts of NaOH used in the reaction with the HCl solution and with the HC2H3O2. I ...
April 21, 2007 by Rachel

chem-acid-base titrations
Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. a.write a balanced equation for this neutralization reaction b.what is the molarity ...
April 21, 2008 by natash

chem
Ok so i looked at it and tried to figure out the conj. base and acid. Are these right? 1) S2-(aq) + HCl(aq) <=>Cl1-(aq) + HS1-(aq) This is what I think it is: Acid = HCl Base = S^2- Conjugate acid =HS^1- Conjugate base = Cl^1- 2) H2O2(aq) + PO43-(aq) <=>HPO42-(aq...
January 29, 2012 by Erik

chem-acid base titrations
If 20.0mL of .2019M HCI requires 39.63mL of a NaOH solution for complete neutralization, what is the concentration of the NaOH solution? how many significant figures are justified in the answer?
April 7, 2008 by natash

chem
Ok so for question I have to state whether the element/compound is an acid, base, conjugate acid or conjugate base. Can u please tell me if i am correct and help me out with the ones i am unsure what the answer is? 1)S^2-(aq)+HCl(aq)<=>Cl^1-(aq)+HS^1-(aq) This is what I ...
January 29, 2012 by Erik

Chemistry
Predict whether the Ph endpoint is =7 >7, or<7 for each of the following acid-base titrations. Justify you predictions a) hydroiodic acid with sodium hydroxide. b)boric acid with sodium hydroxide c) hydrochloric acid with magnesium hydroxide d) hydrochloric acid with ...
June 13, 2010 by Adeola

College Chemistry
Sodium hydroxide is used extensively in acid-base titrations because it is a strong inexpensive base. A sodium hydroxide solution was standardized by titrating 27 mL of 0.1628 M standard hydrochloric acid. The initial buret reading of the sodium hydroxide was 2.44 mL, and the ...
October 3, 2010 by KELLY

Biochemistry
Calculate how you would make 0.5L of a 0.5M (500mM) acetate buffer at a pH of 4.7. Available is sodium acetate and glacial acetic acid. pH=4.7 pKa of acetic acid=4.76 Not sure if I did this next part right: 4.7=4.76 + log [base]/[acid] -0.06= log [base]/[acid] 10^-0.06= [base...
September 11, 2014 by Nicole

chem
Why are titrations using permanganate performed in acid solution?
April 28, 2010 by help

chem
Why are titrations using permanganate performed in acid solution?
April 28, 2010 by help

chem
Why are titrations using permanganate performed in acid solution?
April 28, 2010 by help

Chemistry130
Can someone please help me with this? Are these substances acids or bases? 1. Tums- Base, right? 2. Vitamin C- Acid, right? 3. Nail Polish Remover- Base or Acid? 4. Coca Cola Pop- Acid, right? 5. Cream of Tarter- Acid, right? 6. Calamine Lotion- Base or Acid? 7. Lemon Juice- ...
October 13, 2009 by Adam

acid and base titrations
what is the pH of a solution prepared by adding 0.50 mol KOH to 1.0 L of 0.30 M HNO3?
November 21, 2010 by jj reddick

chem lab (webwork)
Complete the table below: How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (mL) NaOH HCl NaOH HC2H3O2
April 13, 2010 by need help student

CHEMISTRY
What indicator is better in the following titrations : 1) strong acid/strong base a) methyl red (4.4 - 6.2 ) b) bromophenol blue (6.2 - 7.6 ) 2) strong acid/weak base a) methyl orange (3.1 - 4.4 ) b) bromophenol blue (3.0 - 4.6 ) 3) weak acid/strong a) phenolphthalein (8.0 - ...
September 11, 2014 by MAD

Chemistry
When titrating an acid with a base, a dilute solution of the base is used. When titrating a base with an acid, a dilute solution of acid is used. Why are these titrations done with dilute solutions?
October 6, 2010 by Jeff

chem
In the Bronsted-Lowry theory of acids, an acid will lose a proton (H+) and leave behind the conjugate base of the acid. The conjugate base of a strong acid is?
February 19, 2013 by shakira

chem lab (webwork)
How much 0.10 M Base (in mL) is required to neutralize 8.00 mL of the 0.10 M acid? Base Acid Base Volume (mL) NaOH HCl NaOH HC2H3O2
April 13, 2010 by anonymous

Bio Chem
The pKa of propanoic acid (propionic acid), CH3CH2COOH, is 4.87. Consider an equilibrium mixture of propanoic acid and its conjugate base with a pH of 4.87. Draw the structure of the form (acid or conjugate base) that predominates after a decrease in [H3O ]. Include all ...
September 16, 2014 by Cristy

chemistry
If the acid base reaction HA(aq)+B^-(aq)---> HB(aq)+A^-(aq) <--- has a k = 10^-4,which of the following statements are true & why? (a)HB is a stronger acid than HA (b)HA is a stronger acid than HB (c)HA & HB have same acidity (d)B^- is a stronger base than A^- (e)A^- is ...
January 1, 2010 by chikirshu

chemistry
Do strong acid strong base titrations have a buffer region?
May 12, 2011 by jam

Chemistry
Use the Bronsted-Lowry definitions to identify the two conjugate acid-base pairs in the following acid-base reaction: HCO3^- + S^2- <-> HS^- + CO3^2- I got it. HCO3^- is the base in the pair with CO3^2-. S^2- is the acid in the pair with HS^-. Would you believe you have ...
May 26, 2007 by Raj

Organic chem
Classify each as a lewis acid or lewis base... A)H20 B)O2- C)Cu2+ D)SO3 E)AlCl3 Lewis acids are electron pair acceptors. Lewis bases are electron pair donors. Look at H2O, for example. .. H:O: .. H This molecule has no "holes" to accept an electron. Would you expect this to be...
October 15, 2010 by Adam

acid and base titrations
in a titration, 0.0400 mol of solid NaOH is required to neutralize 10.0 mL of H2SO4(aq). From these data, the [H2SO4] is:
November 19, 2010 by jj reddick

Chemistry
my ap chem teacher has been absent for the past two weeks and part of the notes her sub gave us to copy says that In the equation HC2H3O2 + H20 <--> C2H3O2(- charge) + H3O(+ charge) HC2H3O2 is an acid H2O is a base C2H3O2(- charge) is the conjugate base and H3O(+ charge...
May 15, 2010 by Mark

chemistry please check
for the following reactions label each species as an acid or a base. Indicate the species that are conjugate acids and conjugate bases. A. HSO4-(acid) + NH3(base)<--> SO4^2-(conj base) + NH4+ (conj acid) B. HPO4^2- (conj base)+ NH4+ (conj acid) <--> H2PO4-(acid) + ...
April 25, 2010 by Anna

biochemistry
Is CAPS an acid or base? If it is an acid, what is its base? If it is a base, what is its acid? Also, is Tricine an acid or base? If it is an acid, what is its base? If it is a base, what is its acid? Thanks.
January 27, 2008 by stew

chem
How do I calculate ratio of volume of base to volume of acid . Ex) phenolphthalein: Acid:20mL Base 30mL
April 27, 2010 by lou

Chemisty
In titrations of acids and bases, what is the difference between the end point of the titration, and the equivalance point? Also, what is chemically occuring during the buffer zone? Thanks! Good question and one that students sometimes have trouble with. The equivalence point ...
May 15, 2007 by Jessie

chemistry
For each of the following acid-base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 3.60g of the base. 2HNO_3(aq) + Ca(OH)2(aq) -> 2H_2O(l) + Ca(NO_3)2(aq) H_2SO_4(aq) + 2KOH(aq) -> 2H_2O(l) + K_2SO_4(aq) how do i ...
October 20, 2007 by leo

Chem
write the dissociation of acetic acid identifying the base,acid,H donor, and H receiver C2H4O2+H2O - H3O+C2H3O2 is hydronium the H donor and is C2H3O2 the base?
September 6, 2011 by Justin

Chemistry
You have two buffer solutions 1) weak acid and its conjugate base 2)weak base and its conjugate acid. Write explicitly ( considering generic formula for acid and base) the equations of neutralization when you: a) add strong acid and strong base 1) b) add strong acid or strong ...
March 29, 2013 by Grace

Chemistry
I don't know how to reply to an answer. First of all thank you! For the question I just asked about the titration curves. Would that mean that titrating with barium hydroxide would take half the volume that is used when titrating with sodium hydroxide? Oh and there was a ...
March 6, 2012 by Niki

Science
I need help describing the difference between Arrhenius acid/base, Bronsted/Lowry acid/base, and Lewis acid/base. Everything online is too complicated! Thanks!
December 18, 2007 by Janissa

acid and base titrations
Which of the following solutions should be used when titrating a 25.00mL sample of CH3COOH that is approximately 0.1 M? a.) 0.150 M NaOH b.) 0.001 M NaOH c.) 3.00 M NaOH d.) 6.00 M NaOH
November 21, 2010 by jj reddick

chem 2
indictae the reactant that is a bronsted lowry acid. HCN(aq) +H2O (l)---> H3O+(aq)=CN-(aq) HCN CN- H20 H30 i think it is HCN the weak acid substance which acts as a proton (H+) donor and CN the weak base? You are right. The HCN donates the proton (to H2O) so that makes HCN...
April 30, 2007 by jane

Chemistry Logic
How can I tell a conjugate base from a regular base and a conjugate acid from a regular acid? For example, in: H2O + HONH3 (reversible arrows) HONH2 + H3O+ What is the acid, base, conjugate base, conjugate acid? Is there no base and conjugate base since HONH3 is an acid? The ...
August 3, 2007 by Taasha

chemistry
Hi there, ok, my question stated "Use information from acid/base table and the value of Kw t ocalulate the base ionization constant, Kb, of the following bases: a)hypochlorite ion b) nitrite ion c) benzoate ion I looked at my acid/base table but it only gives values for ...
April 8, 2008 by Jay

Chemistry
If an equal number of moles of the weak acid HOCN and the strong base KOH are added to water, the resulting solution will be acidic, basic or neutral? There is a complicated answer and a sensible answer. Both arrive at the same answer. But here is the logic for the sensible--I...
April 27, 2007 by Joel

Chem 2
What is the approximate value of the K for the neutralization of nitrous acid with ammonia? Ka for the acid is 0.00045 and Kb for the base is 0.000018. Do I multiply Ka*Kb?
February 28, 2008 by Sarah

titrations
I have to find the correct acid-base indicator to use for the following titrations (methyl orange with end point @ pH 4, bromthymol blue with end point @ pH 7, or phenopthanlein with end point @ pH 9). I have several problems given to me, but first I'm trying to figure them ...
May 5, 2007 by Taylor

chem. re+asap!
I got the rest, I just need help on the last one. My first post is down on this page. 6th one:I dont know how to write the equation. It would be acid over base but which is the acid and which is the base? My answer: I got the Ka to be 2.7x10^-1. The equation I got was: C6 H 5 ...
June 19, 2006 by hey.

chem
1. 50.00 mL of an unknown monoprotic acid is titrated with 0.132 NaOH. It takes 25.25 mL of base to reach the equivalence point. Calculate the concentration of the acid.
July 25, 2010 by Anonymous

Chemistry
If two titrations were completed were completed: 1) the titration of HCl with Na(OH) 2)the titration of HCl with Ba(OH)2 (the concentrations of acid and base for both titrations are the same) How would the titration curves of each solution be different? I know what the ...
March 6, 2012 by Niki

Chemistry
What is the pH of the solution created by combining 2.00 mL of the 0.10 M base[ammonia] with 8.00 mL of the 0.10 M acid[acid acid]? I tried this problem so many times, but always got it wrong. It's a weak base and acid titration. but i don't know the method of do this type of ...
April 14, 2008 by HELP Plz

Titrations (chem)
In the titration of a 0.101 M sodium hydroxide solution, 19.02 mL of 0.130 M sulfuric acid solution was required to neutralize the sodium hydroxide in reactions that replace both hydrogen ions of the sulfuric acid. Calculate the number of milliliters of sodium hydroxide ...
April 3, 2011 by Sarah

Chemistry
The following questions relate to acid base reactions. a) What type of reaction is said to occur when an acid reacts with a base.? b) What are the general products of such a reaction? i.e. An acid + a base produces . + .
November 7, 2012 by Many

Chemistry
I don't understand how to work out the volumes of weak acid and strong base to mix to make 1L of buffer when given the concentrations of weak acid and strong base (in my case 0.160M NaOH and 0.200M H3PO4) and the pH required (7.00). Specifically the textbook is Fundamentals of...
March 30, 2008 by Sarah

Chemistry
I don't understand how to work out the volumes of weak acid and strong base to mix to make 1L of buffer when given the concentrations of weak acid and strong base (in my case 0.160M NaOH and 0.200M H3PO4) and the pH required (7.00). Specifically the textbook is Fundamentals of...
March 30, 2008 by Sarah

Acid/Base Chem
Determine the volume (in mL) of 1.18 M perchloric acid (HClO4) that must be added to 747 mL of 0.976 M sodium hydrogen citrate (Na2C6H6O7) to yield a pH of 4.77.
March 30, 2011 by Sam

Chemistry
Determine whether each of the following salts will form a solution that is acidic, basic, or pH-neutral? Al(ClO4)3-Acid LiCl-Neutral KClO2-BAse C6H5NH3NO2-Acid CH3NH3Br-Acid KCl-Neutral NaClO-Base NH4ClO-Acid Fe(ClO4)3-Acid C2H5NH3NO3-Acid Is this right?
October 23, 2010 by Anonymous

Chemistry
Determine whether each of the following salts will form a solution that is acidic, basic, or pH-neutral? Al(ClO4)3-Acid LiCl-Neutral KClO2-BAse C6H5NH3NO2-Acid CH3NH3Br-Acid KCl-Neutral NaClO-Base NH4ClO-Acid Fe(ClO4)3-Acid C2H5NH3NO3-Acid Is this right?
October 23, 2010 by Anonymous

college chem
A 0.1276 g sample of a monoprotic acid (molar mass = 1.10 x 10^2) was dissolved in 25.0 ml of water and titrated with 0.0633 M NaOH. After 10.0 ml of base has been added, the pH=5.47. What is the Ka for the acid?
March 28, 2011 by Angelina

pH- part 2
how much .10M Base (in mL) is needed to neutralize 8.00mL of .10M Acid? base- NaOH, acid- HCl, base volume (mL)- ? base- NaOH, acid- HC2H3O2, base volume (mL)- ? VaNa=VbNb Vb= 8ml*.10N/.10N= 8m.
April 14, 2007 by Christine

Chemistry (Titration Curves)
Which of the following Acid+Base titration combinations would have a buffering region in their plot? 1)Strong Acid+Strong base (HCl+NaOH) 2)Weak acid and strong base (Acetic+NaOH) 3)Strong Acid and weak base (HCl+NH3) 4)Weak Acid and weak base (Acetic+NH3) In all cases, there ...
May 8, 2011 by Anonymous

Chem
What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH<--> C6H5COOH Once I get ...
February 27, 2008 by Sarah

Chem
A tank car containing concentrated HCL (molarity 12.1) derails and spills exactly 1500 L of acid. Solid potassium hydroxide is required ot neutralize the spill. (a) Write a balanced chemical equation. HCl + KOH -> kCl + H2O (b) What is the molar ratio between acid and base...
July 6, 2009 by Lena

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

Chemistry
Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Identify the acid and base. Explain how the equilibrium is shifted as buffer reacts with an acid and reacts with a base.
January 24, 2013 by Raphael

CHEM REPOST...PLEASE CHEK!
Posted by Kat on Monday, March 2, 2009 at 11:21am. A solution of volume 80.0 mL contains 16.0 mmol HCHO2 and 9.00 mmol NaCHO2. If 1.00 ml of 12 M HCl is added to this, what will be the resulting pH? Responses * CHEM HELP...PLEASE!! - DrBob222, Monday, March 2, 2009 at 1:25pm ...
March 2, 2009 by Kat

CHEMISTRY
Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number of moles of acid ...
November 9, 2011 by Alexander

Chemistry
Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number of moles of acid ...
November 9, 2011 by Alex

chemisty
600 mL of an unknown monoprotic acid was titrated with a standard solution of a 1.0 M base. If it took 40.0 mL of the base to neutralize the acid, what was the H+ ion concentration of the acid in moles per Liter?
December 14, 2010 by ana

chem
Classify each of the following reactions in as many ways as possible. (Select all that apply.) CuO + 2 HCl --> CuCl2 + H2O you can select: -acid-base(unsure because there is an acid but im not sure if theres a base) -double-displacement -gas evolutionx -oxidation-reduction ...
November 30, 2010 by hannah

chem+Acid-Base Reactions
Hey..can you check this for me. It has to do with Predicting Acid-Base Reactions. So here it is: I have to: Predict the most likely acid base reaction(s) that occur. For each reaction, state if the reaction is quantitative, or, if not, state whether products or reactants are ...
July 25, 2006 by blank

chem
classify each of the following as a lewis acid or base: Cl- BeCl2 B(CH3)3 P(Ch3)3 Cl- is an acid right? i'm not sure i understand this concept very well. :[ and i tried looking at my notes already.
March 28, 2010 by Katie

Chemistry
What effect would be on the normality of unknown acid? Explain why. a) if NaOH solution is pipetted into a conical flask containing some distilled water b) if an air bubble is out from the burette c) if too much acid is ran out during both titrations although the volumes of ...
May 15, 2014 by Peter M.Shaker

CHEM
is NH3 a base or an acid how do u tell?
November 20, 2008 by brian

chem
A beaker with 120mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.70mL of a 0.450M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid ...
July 22, 2013 by pablo

Chemistry
This a back-titration problem, the equation is (mass/molar mass * na)+ (Ma * Va* na) = (Mb * Vb* nb. do the na and nb variables refer to the moles of the acid and base, or the moles of H and OH? acid and base acid and base
June 4, 2007 by Tucker

Chemistry
A buffer containing 1.2169 M of acid, HA, and 0.1431 M of its conjugate base, A-, has a pH of 3.96. What is the pH after 0.0017 mol NaOH is added to 0.5000 L of this solution? I can't figure this out for the life of me, i'm sure its just some simple mistake i'm making but can ...
April 2, 2007 by Rafael

chemistry
What is the pH of the solution created by combining 12.00 mL of the 0.10 M base with 8.00 mL of the 0.10 M acid acid: acetic acid base: ammonia
April 9, 2008 by unknown

Chemistry
Use the Bronsted-Lowry definitions to identify the two conjugate acid-base pairs in the following acid-base reaction: H20 + H20 <-> H30^+ + OH^- Let's see what you think on this after the previous post. Just remember, the acid is the one that HAS the H and the base is ...
May 26, 2007 by Raj

chem
For the following reactions, name the Bronsted-Lowry acids and bases. Then name the conjugate acid and bases. H3O+(aq) + CN-(aq) <==> HCN(aq) + H2O I'm really confused on this whole concept even thought it's not really difficult. I said: acids: H3O+ bases: CN- conjugate ...
April 27, 2007 by Chris

Chem
Bronsted reaction HCO3-+HF<--> acid?+base?
February 21, 2014 by Sharon

Chemistry
In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base d.the hydrolysis of the conjugate base of the weak ...
May 26, 2011 by Cheryl

Chem+ASAP+2 fill in the blank questions+ASAP!!!
PLease check this. They are fill in the blank and I just need to know if they are right. Thanks! 9. Compared to a strong acid-strong base titration curve, a weak acid-strong base titration curve has a (higher, lower) __higher___ initial pH value. 10. Compared to a strong acid...
August 8, 2006 by David

chemistry
Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone explain this combination
November 7, 2010 by poet

chemistry
Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone explain this ...
November 8, 2010 by poet

CHEM LAB
Calculate the Molar Enthalpy of Neutralization in kJ/mol of the reaction between a monoprotic acid and a monoprotic base, given the following information: *Make sure you report your answer using the correct sign* The temperature change equals 9.80 degrees C, 50.0mL of 1.00 M ...
November 6, 2013 by BRANDIE

CHEM LAB
Calculate the Molar Enthalpy of Neutralization in kJ/mol of the reaction between a monoprotic acid and a monoprotic base, given the following information: *Make sure you report your answer using the correct sign* The temperature change equals 9.80 degrees C, 50.0mL of 1.00 M ...
November 6, 2013 by BRANDIE

chem
is a formate ion (HCOO-) an acid or a base? how would you know?
November 16, 2007 by mark

college
1) You are given solutions of HCl and NaOH and must determine their concentrations. You use 37.0mL of NaOH to titrate 100mL of HCl and 13.6 mL of NaOH to titrate 50.0mL of 0.0782 M H2SO4. Find the unknown concentrations. Molarity of NaOH and molarity of HCL? 2) Sodium ...
October 4, 2010 by Ashley

Chemistry
1) You are given solutions of HCl and NaOH and must determine their concentrations. You use 37.0mL of NaOH to titrate 100mL of HCl and 13.6 mL of NaOH to titrate 50.0mL of 0.0782 M H2SO4. Find the unknown concentrations. Molarity of NaOH and molarity of HCL? 2) Sodium ...
October 4, 2010 by Ashley

chem(molarity)
a buffer contains 0.010 mol of lactic acid and 0.050 mol of sodium lactate per liter . How do I find the molarity of the acid and base?
September 9, 2012 by mary

chem
show why ka(kb)=kw for this pair of conjugate acid-base: H2C6H6O6 and HC6H66 ^-1
May 5, 2012 by nicole

Chemistry
A student titrates 0.100M KOH into 50.00 ml of weak acid HX. The pH of the solution is 4.25 after 20.00 ml of the base has been added, and equivalence point is reached when 40.00 ml of the base is added. 1. What is the concentration of the acid, HX ? 2. What is the Ka value of...
March 9, 2011 by Paul

chem
I need major help im not understanding this at all: Complete and balance each of the following equations for acid-base reactions. (Type your answer using the format CO2 for CO2 and Al(OH)3 for Al(OH)3. Use the lowest possible coefficients.) HBr(aq) + LiOH(aq) -> find this ...
November 23, 2010 by hannah

chemistry
do we have buffering region and ph=pka in any of these conditions: strong base vs strong acid strong base vs weak acid weak base vs strong acid weak base vs weak acid
May 23, 2010 by eng

Acid-base titration
A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0, 1, 5, 9, 9.9, 10, 10.1, and 12 mL.
January 23, 2012 by Patrick

chemistry
A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following statements best explains your prediction? 1. ...
March 31, 2014 by bekah

chem
the pH of a .100 M solution of sodium formate = 8.37. Calculate the value of Ka of formic acid. okay so I know that the anion of a weak acid is itself a weak base so A- +H2O---> OH- + HA pOH =14-8.37 so conc of OH is 10^-5.63 Ka=[OH][HA]/[A-] so we know the conc of OH and A...
May 13, 2009 by Natash

Chemistry
Acid is a proton donor and base is a proton accepter? first of all, please respond to this, i have a huge test tomorrow and would appreciate any help i can get! According to the Bronsted- Lowry model, acid gives a proton in an acid reaction and the base takes the proton... ...
March 25, 2009 by Dana

chemistry
Strong base is dissolved in 665 mL of 0.400 M weak acid (Ka = 3.69 10-5) to make a buffer with a pH of 3.94. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -> H2O(l) + A-(aq) Calculate the pKa value of the acid and determine the number of...
July 8, 2012 by craig

chem
Calculate the pH of 0.20 M NaCN solution. NaCN ---> Na+ + CN- CN- + H20+ ---> HCN+ + OH- Initial conc. of CN- = 0.20 mol/L change = -x equillibrium = 0.20-x HCN equill. = +x OH equill. = 1x10^-7+x Ka= 6.2 x 10^-10 Kb = KW/Ka = 1x10^-14/6n2 x 10^-10 = 1.6 x 10^-5 1.6 x 10...
July 24, 2009 by Lena

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