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April 18, 2014

Search: Lakes that have been acidified by acid rain can be neutralized by the addition of limestone (CaCO3). How much limestone in kilograms would be required to completely neutralize a 5.2 x 109- L lake containing 5.0 x 10-3g of H2SO4 per liter?

Number of results: 139,950

chemistry
Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone in kilograms is required to completely neutralize a 5.8×109 L lake with a pH of 5.6? thanks
Saturday, December 4, 2010 at 8:43pm by amy

chemistry
Lakes that have been acidified by acid rain can be neutralized by the addition of limestone How much limestone in kilograms would be required to completely neutralize a lake containing of H2 per liter? 5.0 * 10-3 g SO4 5.2 *
Thursday, July 21, 2011 at 7:54pm by Anonymous

chemistry 101
Lakes that have been acidified by acid rain can be neutralized by the addition of limestone (CaCO3). How much limestone in kilograms would be required to completely neutralize a 5.2 x 109 L lake containing 5.0 x 10-3 g of H2SO4 per liter?
Friday, July 8, 2011 at 9:11pm by ABCD

Chemistry
Lakes that have been acidified by acid rain can be neutralized by the addition of limestone how much limestone in kilograms would be required to completely neutralize a 5.2 x 10^7 -L lake containing 5.0 x 10^(-3) g of H2SO4 per liter.
Monday, May 2, 2011 at 5:05pm by Jarred

Chemistry (again)
Lakes that have been acidified by acid rain can be neutralized by addition of limestone (CaCO3) . How much limestone in kilograms would be required to completely neutraluze a 5.2 x 10-l lake containing 5.0 x 10 g if h2so4 per liter?
Monday, April 23, 2007 at 2:36pm by Robbie

chemistry
Please help!... Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. Write ionic and net ionic equations to show how limestone reacts with HNO3 and H2SO4 to ...
Tuesday, October 12, 2010 at 8:30pm by Anonymous

chemistry
Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1...
Tuesday, October 12, 2010 at 8:30pm by Anonymous

chemistry
Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3) is added to the acidified water. What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1...
Tuesday, October 12, 2010 at 8:30pm by Anonymous

Science
Why do lakes lying in granite basins tend to become acidified by acid rain more readily than lakes lying in limestone basins?
Tuesday, March 11, 2008 at 1:58am by Nancy

Biology
I would say maybe, it could be due to the water temperature, against other lakes should betested as well. What would you say. I would also test against other lakes that have acid rain via non acid rain lakes as well.
Saturday, August 20, 2011 at 7:42pm by Betty

acids and alkalies
I would never use a strong alkali to neutralize an acid (strong acid OR weak acid)BECAUSE an excess of strong alkali after the acid has been neutralized is just as corrosive as the acid might have been had it been left alone. I would use something like sodium bicarbonate (...
Wednesday, April 2, 2008 at 2:17pm by DrBob222

Chemistry
Which of the following is an example of a physical change ? A) Zinc metal is added to hydrochloric acid and a gas is released. B) Concentrated hydrochloric acid is diluted with water. C) Acid rain causes the decomposition of a marble statue. D) Hydrochloric acid is neutralized...
Thursday, December 30, 2010 at 5:35pm by Anonymous

science
Is acid rain a homogeneous or heterogeneous mixture? If we mean that each drop of rain may not have the same amount of acid in it as the next drop, it must be heterogeneous. That would mean that each drop of rain absorbed different amounts of the appropriate oxide(s) forming ...
Tuesday, January 16, 2007 at 9:42pm by Bobby

chemistry
For the titration of 50.00 mL of 0.1000 M ammonia with 0.1000 M HCl, calculate the pH (a) before the addition of any HCl solution, (b) after 20.00 mL of the acid has been added, (c) after half of the NH3 has been neutralized, and (d) at the equivalence point.
Wednesday, April 11, 2012 at 6:03am by chamy

science
Are there any connections between evolution and environmental science-- if there is, what is it? Thanks! Weren't many lakes back in time very acid? I wonder if acid rain is favoring certain mutations in organisms? Will that affect evolution? I didn't quite understand what you'...
Saturday, September 16, 2006 at 12:28pm by Jin

chemistry
A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized? The equilibrium constant (Ka) for acetic acid is 1.8x10^-5
Saturday, July 24, 2010 at 1:31pm by eric

Social Studies
Ships from the Great Lakes travel the St Lawrence river to what ocean? Answer these questions with true or false The five great lakes are large enough to be called inland seas False? The great lakes form north americas most important waterway true? The great lakes have only ...
Monday, November 12, 2012 at 6:17pm by Jerald

Chemistry(Dr.Bob222)
For an acid to be neutralized it means that all of the H^+ has been reacted and there is neither an excess nor a deficiency. For a base to be neutralized it means that all of the OH^- has been reacted completely and there is neither an excess nor a deficiency. It does not mean...
Wednesday, November 20, 2013 at 10:27pm by DrBob222

ap chem
Acid rain has a pH value of 3.0, whereas normal rain has a pH value of 5.6. Calculate the ratio of the hydronium ion in acid rain to that in normal rain.
Monday, February 14, 2011 at 12:21am by Anonymous

ap chemistry
Acid rain has a pH value of 3.0, whereas normal rain has a pH value of 5.6. Calculate the ratio of the hydronium ion in acid rain to that in normal rain.
Thursday, February 28, 2013 at 9:47pm by cheri

Chemistry...Help?
I believe the answer to part (B) can be found in your text in the chapter on Acid Rain. It that chapter, it states that Carbonic Acid acts in the environment to keep rainwater at a pH of between 5 and 7. It then goes on to dicuss the term acid rain as pertaining to ...
Tuesday, May 12, 2009 at 9:03am by Beth

PHYSICS
What causes acid rain? Can you think of a way acid rain could be produced even without industrial pollution? [Hint: Plants produce carbon dioxide, Co2, which reacts with rainwater to produce bicarbonate ions, HCO 3-.] Give one reaction that produces acid rain using industrial ...
Friday, November 30, 2012 at 1:32pm by Aaa

ChemChem
Yes, but delete the phrase "due to acid rain". Very few acid soils are due to acid rain.
Monday, November 2, 2009 at 4:29am by bobpursley

Life orientation
land pollution is 1 of the biggest issue w have in S.A bcoz pipo keeps on polluting the land by dumping thngs dat r harmful 2 the land & that leads acid rain then obvious the plants will die bcoz of that acid rain
Saturday, June 11, 2011 at 12:47pm by nomcebo zwane

Chemistry
The pH of healthy lakes is around 6.0. Due to acid rain, the pH of our lakes & rivers is decreasing. At low pH levels, producers such as phytoplankton cannot thrive. Decreased plankton can cause consumer populations to crash. The end result is a lake devoid of life. If the pH ...
Sunday, December 16, 2007 at 12:12am by Lucy

Geography
This is a question about acid rain, in Canada in particular. Acid rain is an issue in eastern Canada, but not as prevalent in western Canada, due to the fact that the east is more heavily populated and industrialized, so... If acid rain fell evenly across Canada, why would ...
Monday, January 24, 2011 at 5:39pm by cel

Science - 6th grade : CHECK MY ANSWER
Which of the following sets of terms is associated with air pollution caused by burning fossil fuels 1.acid rain, ozone hole, skin cancer 2.methane, smog, carbon dioxide 3.sulfur dioxide, smog, chlorofluorocarbons 4.carbon dioxide, smog, acid rain MY ANSWER: Is the answer: 4....
Saturday, January 18, 2014 at 11:16am by Katalina

social studies
How many lakes does the National Trust in England have? It's hard to find the information about that on the Internet. About 136 lakes or 500 lakes? Would you let me know that or the website? Thank you.
Thursday, October 18, 2012 at 9:03pm by rfvv

Acid/Base chemistry
If the pH of rain water is 5.6 on average what is the concentration of carbonic acid in rain water?
Thursday, April 26, 2012 at 11:09pm by Anonymous

Acid/base chemistry
if the pH of rain water is 5.6 on average what is the concentration of carbonic acid in rain water?
Thursday, April 26, 2012 at 11:11pm by Anonymous

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

Geography
Canada's industry is concentrated in the southeastern part of the country -- along the St. Lawrence River and Lakes Huron, Erie, and Ontario. The smoke from these industries help produce acid rain. The northern tundra region is probably the least affected because it has no ...
Monday, January 24, 2011 at 5:39pm by Ms. Sue

Biochemistry
Use the Henderson-Hasselbalch equation. Th e mixture you have indicated will react to form a buffer, the base will be the sodium lactate and the acid will be the lactic acid not neutralized by the NaOH. Post your work if you get stuck.
Sunday, January 11, 2009 at 9:42am by DrBob222

science
A. Both lye and ammonia are bases; no go. B. Both vinegar and battery acid are acids; no go. D. Both rain water and distilled water are water and not likely to neutralize anything, although rain water sometimes is acidic due to acid rain. no go. C. calcium carbonate and ...
Friday, October 22, 2010 at 7:43pm by DrBob222

chemistry
Henderson equations deal with a weak acid or base salt. Here that is Not the case. the lye neutralized half the acid...so you have started with a volume of .050liter. Moles of acid was .1*.050=.005 moles. You are left .0025 moles acid in a volume of .075 liters (you added 25ml...
Friday, May 23, 2008 at 2:18pm by bobpursley

CHEMISTRY
1.Chemistry Question: A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized? The equilibrium constant (Ka) for acetic acid is 1.8x10^-5 2. Chemistry question: On average, how far is a molecule of air ...
Saturday, August 21, 2010 at 12:28pm by Gerald

Chemistry
Can anyone give me 5 facts everyone should know about acid rain and 5 facts scientists could tell you about acid rain?
Wednesday, October 3, 2007 at 3:31pm by Anonymous

Social studies
Posted by rfvv on Thursday, October 18, 2012 at 9:03pm. How many lakes does the National Trust in England have? It's hard to find the information about that on the Internet. About 136 lakes or 500 lakes? Would you let me know that or the website? Thank you. •social studies - ...
Friday, October 19, 2012 at 12:23am by rfvv

Chemistry Check
yes, correct. Bromic acid would have been HBrO3. Bromic acid is a ternary acid, Hydrobromic acid is a binary acid.
Tuesday, June 22, 2010 at 9:08pm by bobpursley

APChem
You are right about C. A can use the C2H3O2 ion to form HC2H3O2 (acetic acid) and now you have the weak acid and its salt. B is RbOH and HBr. RbOH is a strong base (think NaOH). HBr is a strong acid (think HCl). That's the main reason B can't be a buffer. D is a buffer because...
Sunday, March 21, 2010 at 10:38pm by DrBob222

Science
Why is rain normally acidic, what creates acid rain? Also What is SAV? THANKS!!
Monday, May 24, 2010 at 5:40pm by smiley face

science
When automobiles burn gasoline, they release many pollutants including sulfur oxides into the air. The release of sulfur oxides is a chief cause of acid rain. Which of the following is a consequence to the natural environment due to acid rain?
Wednesday, August 29, 2012 at 3:04pm by Anonymous

bio101
Carbon dioxide forms a weak acid called carbonic acid when dissolved in water. How can this be a significant factor in the formation of acid rain?
Tuesday, August 6, 2013 at 12:59pm by merry

PKA VALUES
I understand that the pH at the half equivalence point gives is the pKa value but could someone explain why this point is the pKa value? HA is a weak acid. HA ==> H^+ + A^- Ka = (H^+)(A^-)/(HA) Solve for (H^+)= Ka*(HA)/(A^-) If we start with, say, 0.1 M HA and start ...
Friday, March 2, 2007 at 4:03pm by amy

chemistry
The formula weight of an acid is 82. In a titration, 100cm3 of the solution of this acid containing 39g of this acid per litre were completely neutralized by 95 cm3 of aqueous naoh containing 40g of naoh per litre. What is the basicity of this acid? Bob helps me
Sunday, March 10, 2013 at 4:46pm by Fai

chemistry
please help solve this problem now. I really need an answer. thank you When one mole of KOH is neutralized by sulfuric acid, q=-56kJ. At 22.8 C , 25.0 mL of 0.500 M H2SO4 is neutralized by 50.0 mL of 0.500 M KOH in a coffee-cup calorimeter. What is the final temperature of the...
Saturday, March 3, 2012 at 7:08am by ogi

4th grade
No. I don't know where you see Lake of the Woods on the map above. However, it has five lakes the form part of the boundary. What do we call these lakes as a group? What are the names of each of these five lakes?
Tuesday, August 4, 2009 at 7:46pm by Ms. Sue

Changes in Matter
Which of the following geological changes are physical changes and which are chemical changes? a)formation of a limestone cave b)creation of a canyon by a river c)wearing of rocks by wave action d)destruction of lakes by acid rain e)heaving of the ground by ice formation a = ...
Monday, March 22, 2010 at 7:26pm by Sara

Asia - JAPAN- Pollution
Hi, I have got a question about Japan's geography; In which ways has the actions of man ( people) affected Japans land? I mean like acíd rain, carbon dioxide etc.( negative effects on the country) I've been googling it, but I can´t find anything. Bea
Monday, May 24, 2010 at 12:59pm by Beatrice

Chemistry
Please help. Calculate the pH at the following points during the titration of 100.0 mL of 0.20 M acetic acid (Ka for acetic acid = 1.8 x 10-5) with 0.10M sodium hydroxide 1. before addition of any base 2. after addition of 30.0mL of base 3. after addition of 100.0mL of base 4...
Tuesday, April 26, 2011 at 5:25pm by Kendall

Chemistry
Calculate the pH at the following points during the titration of 100.0 mL of 0.20 M acetic acid (Ka for acetic acid = 1.8 x 10-5) with 0.10M sodium hydroxide 1. before addition of any base 2. after addition of 30.0mL of base 3. after addition of 100.0mL of base 4. after ...
Monday, April 25, 2011 at 2:25pm by Michael

Chemistry
Can someone check my answers? Thanks. 1.) If you were involved in an acid rain monitoring project with several other samplers, why would it be important that all of you collect your samples on the same day and do the alkalinity tests within 24 hours? Acid rain on another day ...
Wednesday, March 21, 2007 at 6:04pm by Joe

chemistry
Yes to the first question. (H^+) = 10^-pH. At the half way point, which is what you had, then Ka = (H^+ or pKa = pH but that is only true at the half way point. You can see for a weak acid, such as HA HA ==> H^+ + A^- and Ka(H^+)(A^-)/(HA). Solving for (H^+) we get (H^+) = ...
Thursday, April 17, 2008 at 3:04pm by DrBob222

College Chem
if the pH of rain water is 5.6 on average what is the concentration of carbonic acid in rain water?
Thursday, April 26, 2012 at 11:09pm by Anonymous

check
the term reforestation refers to planting new trees: A)where forestlands have been stripped and cleared. B)in old growth forests that have never beeen cut. C)in public lands that have been reclaimed for forsetry d)during the winter months when the rain are light my choose a
Friday, August 21, 2009 at 9:45pm by henry

Chemistry
I have a 1L solution of 0.02M sodium acetate and 0.02M acetic acid. What is the pH after the addition of 0.05 moles of hydrochloric acid? I know this is a buffer question but I have no idea how I am supposed to go about getting the answer... I know Ka values for acetic acid, ...
Thursday, March 4, 2010 at 3:01pm by Alex

chemistry 1A
If 0.2178 g of a diprotic solid acid is neutralized by 44.81 mL of 0.0953 M NaOH, calculate the molar mass of the solid acid
Tuesday, November 2, 2010 at 12:45pm by Jake

chemistry
If an aqueous solution of sulfuric acid (H2SO4) is neutralized by 3.20 mol of sodium hydroxide (NaOH), how many moles of acid were originally present in the solution?
Tuesday, May 10, 2011 at 12:15pm by Anonymous

Chemistry check
Can someone check my answers? Thanks. 1.) If you were involved in an acid rain monitoring project with several other samplers, why would it be important that all of you collect your samples on the same day and do the alkalinity tests within 24 hours? Acid rain on another day ...
Wednesday, March 21, 2007 at 7:25pm by Joe

CHEMISTRY
I think it is easier if you assume some arbitrary number for the volume of acetic acid. Something like 100 mL. moles acetic acid = M x L. moles NaOH when 60 mL acetic acid have been neutralized = M x L. Then use the Henderson-Hasselbalch equation to solve for pH. 2. I would ...
Saturday, August 21, 2010 at 12:28pm by DrBob222

chem
7.50gram quantity of a diprotic acid was dissolved in water and made up to exactly 250ml. If 25ml of this solution were neutralized by 11.1 mL of 1.0 M KOH then what is the molar mass of the acid? I did 7.50/5.55x10^-3
Saturday, July 24, 2010 at 2:18pm by Jin

chemistry
If 8.72 grams of oxalic acid, H2C2O4, a diprotic acid, is neutralized when 23.4 mL of a solution of KOH is added, what is the molarity of KOH? the topic is acid-base triation, and i have already converted the mass to moles,but I am having trouble finding the volume for the ...
Tuesday, April 9, 2013 at 10:10pm by K

Chemistry
Stomach acid is 0.02M HCl. A 330mg antacid tablet is 41% magnesium hydroxide and 36.2% sodium Bicarbonate. What is the volume of acid that can be neutralized by one tablet?
Saturday, May 21, 2011 at 11:54am by Alex

Chemistry
Stomach acid is 0.02M HCl. A 330mg antacid tablet is 41% magnesium hydroxide and 36.2% sodium Bicarbonate. What is the volume of acid that can be neutralized by one tablet?
Saturday, May 21, 2011 at 5:45pm by Alex

Chemistry
You have the Ka for the weak acid is Ka = (H^+)(A^-)/(HA) If we solve this for (H^+) we get ((H^+) = Ka*(HA)/(A^-) At the exact half-way mark to the equivalence point, the acid that is left (not yet neutralized) exactly equals the salt formed; therefore, (HA) = (A^-). Thus, (H...
Friday, March 12, 2010 at 7:28pm by DrBob222

science
All bodies of water collect rain -- reservoirs, rivers, streams, lakes, oceans, seas, bays, gulfs, creeks.
Monday, May 4, 2009 at 5:17pm by Ms. Sue

Chemistry
The ICE thing is difficult to show on these boards because we have a problem with spacing. But I think I can show you. I re-read the problem and I think it means something different. I think it should have said, "what volume of ACID (not base) is required to reach the ...
Sunday, April 6, 2008 at 6:19pm by DrBob222

Chemistry
Calculate the acid concentration of a sample of acid rain with a pH of 4.20
Thursday, August 4, 2011 at 6:05pm by Domenic

Chemistry
Calculate the acid concentration of a sample of acid rain with a pH of 4.20
Thursday, August 4, 2011 at 6:06pm by Domenic

Science
Calculate the acid concentration of a sample of acid rain with a pH of 4.20
Thursday, August 4, 2011 at 6:32pm by Domenic

biology
Research the sea lamprey, an exotic species that has had a great impact on the fish communities of the Great Lakes. a) Describe the niche of the sea lamprey. b) Find out how sea lampreys may have entered the Great Lakes ecosystem. c) Identify the interspecific interactions of ...
Wednesday, August 11, 2010 at 5:19am by peter

Introductory Chemistry
In a titration 25.1ml of a monoprotic weak acid is neutralized with 25.1 ml of .502M NaOH(aq). Calculate the Ratio of [A-] to [HA] after 12.55 of the .502 M NaOH has been added to the initial amount of HA. Anyone have any idea what's going on. I got as far as to find the mol's...
Wednesday, February 4, 2009 at 8:12pm by Nina

Chemistry
Use the Henderson-Hasselbalch equation. However, you will note that the acid is exactly half neutralized; therefore, the base and acid terms will cancel to leave 1, the log of 1 is zero and pH = pKa for an answer but you work it out to see.
Monday, October 18, 2010 at 11:44pm by DrBob222

DrBob222 : need help with the problem
Suppose you have 100 mL of 0.1M H2SO4. You titrate it with 0.1M NaOH. It takes 10 mmols NaOH to neutralize the first H ion AND it takes 10 mmols of NaOH to neutralize the second H. So after you neutralize the first H you STILL have 10 mmols of H to neutralize. That's what I'm ...
Tuesday, September 11, 2012 at 12:55am by DrBob222

Check out my anwser for this science question plez
The chemicals make rain acidic how does it happen? Is it this it? The chemicals from the black smoke gets mixed up in the water cycle and creates acid rain.
Sunday, October 21, 2007 at 5:21pm by Vero

Chem. Again
28: You have a glass of pure water. Are chemical reactions occurring in the water? If so, what are they? If not, explain why not. 29: While investigating the effects of acid rain in your area, you discover a lake that is surprisingly resistant to changes in pH caused by acid ...
Tuesday, May 12, 2009 at 11:30am by Rachel

chemistry
The secret to these titration problems is to know where you are on the titration curve. Let's call the acid HBu. HBu + NaOH ==> NaBu + H2O mmoles HBu = M x L = 20.00 mL x 0.1 = 2 mmoles. mmoles NaOH = M x L = 26.5 mL x 0.1 = 2.65. It should be obvious that all of the HBu ...
Sunday, October 31, 2010 at 8:41pm by DrBob222

chemistry
calculate the number of g fes04 that will be oxidized by 24ml of a 250N Kmn04 in a solution acidified with sulfuric acid. The unbalanced equation for the reaction. The answer 0.912g Who helps
Saturday, February 9, 2013 at 5:58pm by Fai

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

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

5th grade social studies
What are the geographical features of your community or region? Do you have flat, fertile land? Do you have big hills or mountains? Do you have a lot of lakes -- or are near the Great Lakes or an ocean? Do you have a river? Please tell us about the geographical features of ...
Sunday, November 7, 2010 at 6:26pm by Ms. Sue

Chemistry
It isn't irrelevant and it makes a lot of sense. I have been asked this dozens of time in class and many students wonder how the volume of the water added makes no difference. Two ways to explain it. The most scientific way is this way. Say we titrate 25 mL 1.0 M acid with 25 ...
Wednesday, May 9, 2012 at 8:37pm by DrBob222

Gr 11 chem
hydrofluoric acid to be neutRalized
Friday, November 13, 2009 at 5:26pm by chental

acids and alkalis
Nearly everythings an acid or alkali. ( ) (~~~~~~~~~~) Theres Rain. ......... ...... ... Hydrochloric acid. Dno where that comes from but it rings a bell!!!! Hope I could help bbz.
Saturday, November 4, 2006 at 5:56am by W o O p

Biology
I had to think about your question for a bit. Usually, you add a strong base to see an increase in the pH for a titration, but in this experiment you added a strong acid and saw an increase in the pH; this should not have been the case. It seems as though you were adding a ...
Monday, January 28, 2013 at 1:10pm by Devron

AP Chemistry
a) Use the Henderson-Hasselbalch equation shown on the next line below. b) pH = pKa + log[(base)/(acid)] When the solution is diluted you change the base concn and you change the acid concn but does the ratio change? c) Addition of HCl increases concn acid and decreases ...
Sunday, April 25, 2010 at 12:24pm by DrBob222

Chemistry
Why can a buffer be created by the addition of sodium hydroxide to acetic acid, but not from the addition of sodium hydroxide to hydrochloric acid?
Sunday, March 4, 2012 at 8:39pm by Lindsey

Chemistry Help?
Since I'm not an expert on air pollution, I won't comment except for a couple of things. First, I think your answers are ok. NO2 seems to fit but I would have thought of other compounds before I thought of NO2. Second, have you considered that there are other pollutants ...
Wednesday, May 13, 2009 at 12:30pm by DrBob222

Chemistry
Buffers are commonly at a neutral pH of 7; this is wrong. Buffers are usually equal to the pKa or pKb of the acid and its conjugate base, or the base and its conjugate acid. You are right: they do counter act the addition of an acid by by making more of its conjugate base, or ...
Thursday, March 14, 2013 at 2:20am by Devron

Chemistry
1.mole of NaOH added = cv = 0.365x15e-3 = 5.48e-3 moles. Reaction; HI + NaOH --> NaI + H2O pH = -log[H+] the [H+] is the concentration of the acid as 15ml NaOH has been added. the equation states that, 1 mole of NaOH neutralize 1 mole of HI. So, after adding 15ml, we ...
Monday, June 3, 2013 at 10:03pm by bonjo

chemistry
Buffers work because of the way they are constructed. Buffers consist of a weak acid and a salt of the weak acid. For example, HF for the weak acid and NaF as the salt. When a strong acid, such as HCl, is added, the multiple H^+ are used up by the salt to form more of the weak...
Friday, May 4, 2012 at 5:14pm by DrBob222

Chemsitry
Hello. I'm not n=sure about these answers so i was wondering if someone could check them out? 27, A: Which is a stronger acid - sulfuric or carbonic acid? (Answer: Sulfuric acid.) 27, B: Imagine you have two glasses. One contains a solution of carbonic acid. The other contains...
Monday, May 11, 2009 at 12:33pm by CRCAWF

English
1. Can you give me a rain check? 2. Can I take a rain check? 3. Can I have a frain check? 4. Can I get a rain check? (Are they all grammatical and the same? Which expression is commonly used?)
Tuesday, November 20, 2012 at 10:01am by rfvv

Chemistry
I feel that it would result in an increase in the apparent percent yield because the actual yield would be larger than what it would have been had the recrystallization been carried out. I think your reasoning is ok and the answer is ok. If you have used all of the salicylic ...
Thursday, April 2, 2009 at 4:29pm by DrBob222

Chemistry
The trick to these problems is to determine what is present in the solution at the point of your calculation. CH3NH2 + HCl ==> CH3NH2*HCl. moles CH3NH2 = M x L = 0.200 x 0.1 = 0.02 moles HCl = M x L = 0.100 x 0.070 = 007. So you will have an excess of CH3NH2 (all of it is ...
Saturday, November 14, 2009 at 3:33pm by DrBob222

Chemistry
Of what concn? If the strong acid and the weak acid have the same molarity, each will require the same number of drops of NaOH for completer neutralization. Remember, the NaOH can't tell that it is neutralizing a weak acid or a strong acid. All it knows to do is to neutralize ...
Tuesday, May 4, 2010 at 9:03pm by DrBob222

Chem--buffers
NaOH is a strong base; it reacts with CH3COOH, a weak acid, as follows: CH3COOH + NaOH ==> CH3COONa + HOH Since you began with 10 millimoles CH3COOH and 5 millimoles of NaOH, you will produce 5 millimols of the salt (CH3COONa) and you will have left over, at equilibrium, 5 ...
Sunday, February 28, 2010 at 7:56pm by DrBob222

chemistry
19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution Please judge my work: Becasue NaOH and acetic acid react in a 1:1 ratio, initital moles of acetic acid =0.0019 L x 0.44M = 0.000836 mols...
Wednesday, April 9, 2008 at 11:03pm by Joseph

Science
For million of years, wind and rain have worn down the earth. The land is not totally level now because ____. a. other forces keep building up the land b. wind and rain cannot erode solid rock c. for most of those years, wind and rain were scarce d. wind and rain pile dirt ...
Thursday, February 24, 2011 at 9:40pm by Emily

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