Search: Ph. Ed

Number of results: 7,368

collefge
At what volume of added acid is the ph calculated
Friday, October 28, 2011 at 3:52pm by ed

math
Ed, Ethan and Nathan are playing a game. Ed has won11 rounds, Ethan has won 8 rounds, and Nathan has won 1 round. Write the relative frequency of Ed not winning a round as a percent. 45%? Is my Answer correct?
Tuesday, March 9, 2010 at 5:31pm by Ed

chemistry
Disadvantage of using pH indicators for what? For titrations it is that not all indicators change at the equivalence point pH. If for determining the pH of a solution, it is because most pH indicators have a pH range of about 2 pH units which isn't very close if you want ...
Wednesday, April 29, 2009 at 8:23pm by DrBob222

Ecconomics
Price elasticity of demand.Tell whether is elastic,perfectly inelastic,perfectly elastic, inelastic,or unit elastic. And what would happen to total revenue if a firm raised its price in each elasticity range identified.a.Ed=2.5 b.Ed=1.0 c.Ed=~ D. Ed=0.8
Sunday, June 18, 2006 at 4:55pm by nora

Chemistry
Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 8:09pm by norma

Chemistry
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 7:26pm by DrewS

Science
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 4:25pm by DrewS

Science
a. (H^+)(OH^-) = Kw -= 1E-14 b. X = pH of 5; Y = pH of 4. c. pH = -log(H^+) Solve for (H^+)l. d. pH < 7 = acid pH = 7 = neutral pH > 7 = basic e. See b and d. f. pH + pOH = pKw = 14; then pOH = -log(OH^-)
Monday, September 10, 2012 at 1:03pm by DrBob222

Chemistry
Okay, so based on the chart in my book I was able to determine the following. pH=(unknown) pKa=7.2 of Phosphoric Acid (2) A-=.5M of Na2HPO4 HA=.3M H2PO4- pH= 7.2 + log(.5/.3) pH=7.2+log(1.6667) pH=7.2+0.5108 So, the pH of this solution is: pH=7.7108 Correct?
Wednesday, July 6, 2011 at 11:13am by Shaun

Chemistry
A = pH of 8. 1,000 times means difference in pH of 3. If it is more H^+, then pH = 5 for the new solution. Is that acid or basic. pH<7 = acid pH=7 = neutral pH>7 = basic
Monday, November 14, 2011 at 3:56pm by DrBob222

Chem
pH = -log(H^+). Since the pH is a log function, the H^+ from 1 pH to the next (either higher or lower) is in steps of 10. That is pH = 2 is 10x weaker than a pH of 1 and 10x stronger than a pH of 3
Tuesday, May 4, 2010 at 8:26pm by DrBob222

science HElp
Ph scale Which on is true A substance with ph is twice as acidic as substance with ph of 4. A subtances with ph 3 is 10 as acidic as substance with ph of 4. A substance with ph 3 twice as alkies as substances with ph 4. a substancs with ph 3 10 time alkies as substance with ph...
Wednesday, November 23, 2011 at 7:14pm by shan

Chemistry
What is the [H+] of a 0.1 M malonic acid with a Ka of 10^-9 solution? I thought it was just (Ka x Ca)^(0.5), but that doesn't get me a pH of 5.
Saturday, May 7, 2011 at 9:34pm by Ed

Chemistry
a. pH = -log(H^+) pH = -log(7E-4) pH = -(-3.15) pH = 3.15 b. pH + pOH = pKw = 14 pH + 6 = 14 pH = 8 The problems asks for (H^+); therefore, pH = -log(H^+) 8 = -log(H^+) -8 = log(H^+) (H^+) = 1E-8
Tuesday, April 30, 2013 at 11:21pm by DrBob222

science
Are the following substances acid, base, or neutral: sodium bicarbonate (pH = 8.3): Blood (pH = 7.4): milk (pH =6.7): orange juice (pH = 3.6): milk of magnesia (pH = 10.5): How do you come up with the answers?
Monday, March 12, 2012 at 3:56pm by long

chemistry
which solution has the highest concentration of hydroxide ions? a ph=7.93 b ph=12.59 c ph=7.00 d ph=9.82 e ph=3.21 i know the answer is 7 but why is it seven? would it be different if it said hydronium ions?
Saturday, December 11, 2010 at 1:07pm by jessie

Algebra
Is this correct? If not can you please tell me what steps I did wrong? Thanks! The hydrogen ion concentration of milk is about 1.6 x 10^-7 moles per liter. Find the pH. pH = -log [H+] pH = -log[1.6 x 10^-7] pH = -(-7.204119983) pH = 7.2 The pH balance of the milk is 7.2
Friday, June 18, 2010 at 8:41pm by Kate

Chemistry
How will the addition of sodium acetate to an acetic acid solution affect the pH? A. solution becomes hotter B. It will lower the pH C. It will raise the pH D. pH will not change E. pH cannot be measured I selected answer D and got it wrong. I don't understand why...
Sunday, March 10, 2013 at 12:18pm by Lisa

Chemistry
thank Dr.Bob222 I see you got the same answer I did. I got one more I need help with if you can help me please Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 5:37pm by norma

chemistry
pH pure H2O = 7 (H^+) = (OH^-) = 1E-7M acid pH < 7 base pH > 7 neutral pH = 7
Sunday, April 21, 2013 at 12:44pm by DrBob222

science
1. Which of the following is TRUE regarding this situation: Solution A has a pH of 7.38, and Solution B has a pH of 7.42? a.Solution B is more acidic than Solution A b.The pH of Solution A falls within the homeostatic pH range for extracellular body fluids, but the pH of ...
Monday, January 28, 2013 at 12:21am by a

chemistry
No, that isn't correct. The more acidic the solution, the lower the pH. pH <7 = acid pH = 7 neutral pH >7 = basic
Tuesday, November 8, 2011 at 6:27am by DrBob222

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks
Thursday, May 5, 2011 at 12:38pm by Renee

Chemistry
How many moles of NaOH must be added to 1.0 L of 2.2 M HF to produce a solution buffered at each pH? (a) pH = pKa (b) pH = 4.24 (c) pH = 4.60
Wednesday, March 13, 2013 at 2:48am by Margaret

AP Chemistry
Refer to your post below. pH = -log(H^+). Substitute and solve for (H^+). pH<7 = acid pH = 7 = neutral pH >7 = basic.
Wednesday, January 9, 2013 at 10:11pm by DrBob222

biochemistry
What is the net charge on Phe-Asp at each pH? a. pH 1 b. pH 7 c. pH 14
Friday, April 27, 2012 at 8:11am by krystal

chemistry
What is the net charge on Phe-Asp at each pH? a. pH 1 b. pH 7 c. pH 14
Thursday, April 26, 2012 at 10:46pm by krystal

Investing
Economyst Good to hear from you again! Thanks, as always for yor hwlp, you explained this alot better than the book did. Much appreciated! Ed
Thursday, July 17, 2008 at 8:06pm by Ed

chem
pH= -log [H+] pH < 7 is acidic and pH > 7 is basic. for example pH= - log [1.0e-11M] pH= 11 therefore basic solution.
Thursday, November 29, 2012 at 10:48pm by michelle

Chemistry
Here is a site that explains what pH is all about and gives a somewhat lengthy explanation of pH and the pH of common chemicals. It goes on to say that there are many factors that control the pH in lakes and that the pH varies with season as well as during the daylight and ...
Monday, May 12, 2008 at 11:48am by DrBob222

biology -urgent...highly confused
How does pH affect the activity of catalase? Consider both high and low pH, and explain your observations by discussing the effect of pH on protein structure. I cannot find anywhere in my notes, or text book, or even on the internet how pH affects catalase. I know that with pH...
Wednesday, February 27, 2008 at 10:08pm by Leo

chem can u check answer please
I'm not ure that that is right... [H+] = -log(pH) however, we are given a pOH, not a pH. pH + pOH = 14 pH = 14 - pOH so 14 - 9.262 = pH pH = 4.738 [H+} = 10^-ph = 10^-4.738 [H+] = 1.8281 x 10^-5 M
Sunday, May 23, 2010 at 10:36pm by Emma

Chemistry-pH
If it's a liquid, I would use a pH meter. A colored sample doesn't necessarily negate measuring the pH with a piece of pH paper (litmus, for example) if the measurement doesn't need to be highly accurate.
Tuesday, January 25, 2011 at 5:12am by DrBob222

BIOLOGY
A SALT IS OBTAINED AS A REACTION BETWEEN A SALT (and water) IS OBTAINED AS A REACTION BETWEEN a base and an acid. See: http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/acidbase.html http://lrs.ed.uiuc.edu/students/erlinger/water/background/ph.html I hope this helps. Thanks ...
Saturday, September 30, 2006 at 12:29pm by CAROLINE

Chemistry
pH = -log(H^+) pH = -log(2) = -(0.301) = -0.301 pH<7 acidic pH = 7 neutral pH>7 basic
Tuesday, May 10, 2011 at 3:48pm by DrBob222

Chemistry 130
pH = -log[H+] The above relationship can also be expressed as: [H+] = 10^(-pH) or [H+] = 1 / 10^(pH) That shows the hydrogen ion concentration is inversely proportional to the pH.
Tuesday, October 13, 2009 at 10:53am by GK

math
Ed Long promised to pay his son $400 semiannually for 12 years. Assume Ed can invest his money at 6% in an ordinary annunity. How much must Ed invest to pay his son $400 semiannually for 12 years? 24 periods, 3% (Table 13.2)
Wednesday, November 16, 2011 at 1:15pm by jackie

chemistry
pH = pKa + log ([A-]/[HA]) pH = pKa + log ([C2H3O2-] / [HC2H3O2]) pH = -log (1.8 x 10-5) + log (0.50 M / 0.20 M) pH = -log (1.8 x 10-5) + log (2.5) pH = 4.7 + 0.40 pH = 5.1 I used this example And I still got it wrong it should have been 4.75 + 0.12 = 4.87 or do I use just 4.7...
Friday, November 11, 2011 at 8:02pm by Monique

Chemistry
I made a couple of mistakes 1: Equation is: pH = pKa + log([A-]/[HA] Notice addition instead of subtraction 2: Change in pH: pH = 4.202 + log(.0096/.0104) pH = 4.167
Thursday, November 1, 2012 at 1:00pm by Anonymous

Chemistry
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.) (a) pH = 4.70 (b) pH = 5.26 (c) pH = 5.42 (d) pH = 4.96
Wednesday, March 13, 2013 at 2:47am by Margaret

Math
Ed long promised to pay is son $400 semiannually for 12 years. Assume Ed can invest his money at 6 % in an ordinary annuity. How much must Ed invest today to pay his son $400 semiannually for 12 years?
Friday, November 11, 2011 at 4:36pm by Anonymous

chemistry
I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5
Monday, April 12, 2010 at 9:18pm by heather

Chemistry
I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5
Monday, April 12, 2010 at 6:42pm by Larry

math
ed needs to purchase 5.6 meters of tape. if each roll contains 80 cm and costs 5.00 what is the total cost of the tape ed must buy
Thursday, March 7, 2013 at 4:10pm by sam

geometry
if ed= x+4, and dm= 3x-8 find ed,dm and eb
Wednesday, October 19, 2011 at 9:13pm by Heath

chemistry
acetic acid: 0.1 M 30ml hydrochloric acid 0.1 M 5 ml sodium hydroxide 0.1 M 15 ml Buffer + 5ml of: 1.91 ph ph (measured): 4:52 ph HOW DO I CALCULATE PH(CALCULATED)? AND ALSO IT SAYS SHOW YOUR CALCULATION FOR THE PH OF THE BUFFER BEFIRE AND AFTER THE ADDITION OF HCL? COULD YOU ...
Saturday, July 14, 2012 at 6:28pm by fenerbahce

maths-Circles
This is clearly wrong. Suppose CD is a diameter of the circle and AB is any other chord. Then ED is the shortest distance from E to any point on the circle. ED≠EB
Tuesday, February 26, 2013 at 1:37pm by Steve

Chemistry
How many moles of NaOH must be added to 1.0 L of 1.4 M HC2H3O2 to produce a solution buffered at each pH? (a) pH = pKa mol (b) pH = 3.07 mol (c) pH = 5.15 mol
Sunday, December 5, 2010 at 3:22pm by justin

MATH
DAN,DEBBIE,ED AND GENE WERE TRAINING FOR CROSS-COUNTRY RACING. ED RAN TWICE AS FAR AS DEBBIE. GENE RAN 8KM LESS THAN ED. DEBBIE RAN 5KM MORE THAN DAN. DAN RAN 6KM.HOW FAR DID EACH PERSON RUN? (HINT START WITH DAN'S DISTANCE AND WORK BACKWARDS)
Tuesday, October 11, 2011 at 4:28pm by STELLA

Chemistry.
pH C ( dark green) pH : 8 d ( purple) pH : 3 Suppose u mix togather equal amounts of the solutions that produced the results of strip C and strip D , then test the pH of this new solution. What colo will the indicator paper be ? Explain.
Saturday, February 23, 2013 at 10:43am by Mia

Chemistry
Second thought I just don't understand what to do. pH= pKa + log [NH3]/[NH4NO3] pH= -l log ? + log (0.005/?) pH= ? pH= ?
Friday, November 11, 2011 at 8:45pm by Monique

Chemistry
Calculate the pH of a 100mL solution of 0.10M acetic acid ka=1.8x10(-5) i calculated the pH to be 2.87 from the square root of (1.8x10(-5) * 0.1, the negative log gives me the pH. The next question wants you to calculate the pH with 50mL HCl added. I found the pH to be 2.78 by...
Tuesday, October 25, 2011 at 12:38am by Kevin

biochemistry with more info that was needed
I don't think pH of 7 is the way to go. I know this is a pre-lab; however, it says you will be given a pH. Look at the procedures part A, Step 1, and see if they don't list a pH for some of those procedures. That will be the pH you want to use. The appropriate acid/...
Sunday, January 27, 2008 at 5:35pm by DrBob222

Chem
You need to learn how to do this. Punch 1.6 x 10^-5 into your calculator. Hit the log button. You should get -4.79588 so the equation now looks like this. pH = -log(H^+) pH = -log(1.6 x 10^-5) pH = -(-4.79588) pH = 4.79588 which rounds to pH = 4.80
Saturday, June 19, 2010 at 11:27am by DrBob222

chemistry lab
Could someone help me with this? i am tired of it. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01 M: 7.42 pH of ...
Friday, February 1, 2008 at 10:54pm by amanda

chemistry
A distribution curve shows how the fractions of non ionized acid and its conjugate base vary as a function of Ph. The curves of the plot of [CH3COOH] vs. Ph and [CH3COO-] vs. Ph will intersect at a Ph of what? I need to show work
Sunday, April 22, 2012 at 1:30pm by court

chemistry
What will be the final pH value if you mix 50ml HCl (aqueous solution, pH=0.5) and 40ml NaOH (aqueous solution, pH=12). Hint: convert pH value to concentration of acids/base, then consider the neutralization reaction, then find out the resulting pH value. Please show me your ...
Thursday, April 4, 2013 at 11:44am by Anonymous

Chem
for hydroxide ion, there's an additional step to find pH. after finding pOH, you'd have to plug it into the second equation and solve for pH. if you were given hydrogen ions, you could find pH in one step. pH= -log(H^+) the concentration of hydrogen ions is essentially...
Tuesday, September 14, 2010 at 5:42pm by TutorCat

chemistry
The definition of pH is: pH=-log[H3O+] An equivalent statement is: [H3O+] = 10^-pH The hydronium concentration is the antilog of the (-pH) For this example, [H3O+] = 10^-10.5 = ?? The definition acid, basic, and neutral pH's should be something you can look up in your ...
Tuesday, July 14, 2009 at 7:10pm by GK

chemistry
sorry 0.1 M NH4OH has pH 9.8 so I need the theoretical pH for 14 - 0.5(pKb-log [base])=? also 0.1 M HAc pH=2.5 theoretical pH 0.5 (pKa-log [acid])= ? Gratefull for help
Friday, June 1, 2012 at 3:24am by lynda

Chemistry
The calculations will be affected a lot by what is in the water already (I assume it is not pure water). You should be testing the water lime mixture for pH, testing is easy with pH paper, and accurate. Any living thing in water affects the pH also, especially with its waste ...
Wednesday, May 7, 2008 at 12:39am by bobpursley

Science
Three acids solutions have the following pH: Solution A: pH = 2 Solution B: pH = 5 Solution C: pH = 3 Which solution is made with the acid that has the smallest ionization constant?
Thursday, June 30, 2011 at 11:14pm by Megan

chemistry
Calculate the pH range required to separate 99.99% of Cr3+ from Zn2+ by precipitation of Cr(OH)3(s) in a solution that is initially 0.034 M in both Cr3+ and Zn2+. Use the Ksp values from Table 16.2 of Chang and calculate the pH to the nearest 0.01 pH unit. Lowest pH= Highest pH=
Sunday, March 25, 2012 at 5:17pm by Tanner

Chemistry
pH pH ( strip c : 8 ) dark green pH ( strip d : 3 ) purple - suppose u mix togather equal amounts of the solutions that produced the results of strip c and d , then test the pH of this new solution. What color will the indicator paper be? Explain .
Sunday, February 24, 2013 at 5:30am by Ruby

chemistry
a. pH = -log(H^+) pH = -log(7.3 x 10^-5) pH = -(-4.14) pH = 4.14 For questions involving OH, just find pOH from the (OH^-), then use pH + POH = 14
Wednesday, January 6, 2010 at 6:36pm by DrBob222

chem101
You're batting 1000 on a. Just plug in the numbers for b and c. b. HCl is a strong acid (meaning it ionizes 100%) so HCl ==> H^+ + Cl^- If HCl = 1.0 M then (H^+) must be 1.0 M (and Cl^- must be 1.0 M). c. pH = -log(H^+) pH = -log(1.0) pH = -(0) pH = 0 (Note: I doubt...
Wednesday, November 28, 2012 at 9:32am by DrBob222

Chem Webwork
Complete the table below: What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water (like it will be in the experiment you perform in lab)? mL NaOH: 0.70 pH w/ HCl: 2.14 pH w/ HC2H3O2: ??? I got pH w/ HCl, but I can...
Monday, April 25, 2011 at 4:25pm by Michelle

Ph. Ed
five (5) different products that have to do with sports. It can be exercise equipment, practice equipment, protective equipment, supplements, etc. Tell me about each product, the price, and if you would or would not but this product and why or why not.
Thursday, April 10, 2008 at 3:26pm by Eagle

chemistry
It isn't pH 6.5. You must determine (H^+) from pH 6 and (H^+) from pH 7, average them, then determine pH from that new (H^+).
Thursday, August 6, 2009 at 6:11am by DrBob222

Chemistry
I suspect the problem is that the question asks for CHANGE in pH and you're giving the data base the pH. I think something like 1.128 which I would round to 1.13 is the answer for the HCl part. I didn't work the NaOH part. pH = pKa + log(9.24/0.7). pH = pKa + 1.128. I ...
Tuesday, March 27, 2012 at 6:01pm by DrBob222

chemistry
How much 6M HNO3 will be required to decrease the pH of 5000L solution of pH=9.6 to pH=3?
Friday, January 4, 2013 at 5:45am by vidya

science
pH = -log(H^+) Substitute H^+ and solve for pH. The answer to the first one is pH = 12
Monday, April 26, 2010 at 6:40pm by DrBob222

chemistry
Who told you the correct answer is 7.00? That isn't right. Reason through it. Low pH means high pOH (since pH + pOH = 14) and that means high H^+. So for high OH^- we want a high pH which means a low pOH and that is a high OH^-. If you don't like that method, go ...
Saturday, December 11, 2010 at 1:07pm by DrBob222

psychology
Ed, who suffers from dementia, has enormous difficulty getting dressed in the morning because he cannot plan and organize the behaviors necessary to complete the task. Ed's difficulty is in the area of A) executive function. B) agnosia. C) apraxia. D) aphasia.
Saturday, December 8, 2012 at 10:44pm by ashley kay

chemistry
I assume you want the pH of the solution. pH = pKa + log(base)/(acid) Substitute and solve or pH.
Wednesday, October 24, 2012 at 8:20pm by DrBob222

chemistry
A water containing 1x10^-4 mol CO2/L and having an alkalinity of 2.5x10^-4 eq/L has a pH of 6.7. The pH is to be raised to pH 8.3 with NaOH. How many moles of NaOH per liter of water are needed for this pH adjustment? (pK1=6.3 and pK2=10.3)
Tuesday, October 12, 2010 at 1:07pm by Ann

Chemistry
Neither K^+ nor Cl^- are hydrolyzed; therefore, the pH is just that of H2O. (H^+)(OH^-) = Kw = 1E-14. Solve for H^+ and convert to pH. pH = 7.00. Note: I assume this is a lower level course; if not that you must calculate the ionic strength of the 1.7M KCl solution and the pH ...
Wednesday, July 4, 2012 at 1:19pm by DrBob222

Chemistry
Let's see. If we dilute 0.1(pH = 1) to 0.01 (pH = 2), is that a decrease in pH? :-) I think it can't be a, b, or c.
Monday, May 20, 2013 at 2:58pm by DrBob222

chemistry
pH = 7 = neutral pH < 7 = acidic pH > 7 = basic
Monday, December 5, 2011 at 2:19pm by DrBob222

Chemistry
pH = 7 is neutral pH<7 = acidic pH>7 = basic
Saturday, July 30, 2011 at 5:37pm by DrBob222

chemistry
1E-5 H^+ = pH = 5 2E-4 H^+ = pH = 3.7 pH + pOH = pKw = 14
Sunday, July 10, 2011 at 1:38pm by DrBob222

chemistry
pH of 3 is acidic. pH of 10.5 is basic. The water is pH of 7 and neutral.
Saturday, June 25, 2011 at 9:48pm by DrBob222

chemistry
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at each of the following. (a) pH 7.7 (b) pH 9.6 (c) pH 11.3
Wednesday, March 27, 2013 at 10:35am by hannah

chemistry
It can. For example, if M HCl = 0.1M, then (H^+) = 0.1 and pH = 1 If M HCl = 1.0, then (H^+) = 1.0M and pH = -log(1.0) = 0 If M HCl = 10.0, then (H^+) = 10.0M and pH = -log(10) = -log(1) = -1. We usually work with pH values for solns in the 0.1 and smaller range; therefore, ...
Sunday, January 22, 2012 at 10:30pm by DrBob222

CHEM
Are you allowed to look up the value for Ka for HClO? If so that makes it easy. If not that presents a problem but I would do it this way. pH = pKa + log(base)/(acid) pH = pKa + log 0.1/0.1 pH = pKa + log 1 pH = pKa + 0 pH = pKa. I may not have understood the question; you may...
Saturday, April 13, 2013 at 3:36pm by DrBob222

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:14pm by fernatesfsdf

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:01pm by JIM

Chemistry
pH=(unknown) pKa=7.2 of Phosphoric Acid (2) A-=.5M of Na2HPO4 HA=.3M H2PO4- pH= 7.2 + log(.5/.3) pH=7.2+log(1.6667) You are ok to here pH=7.2+0.5108 I find 0.22 for the log of 1.6667
Wednesday, July 6, 2011 at 11:13am by DrBob222

biochemistry
a. What is the net charge on valine at pH 1? b. at pH 7? c. at pH 14?
Friday, April 27, 2012 at 8:11am by krystal

chemistry
a. What is the net charge on valine at pH 1? b. at pH 7? c. at pH 14?
Thursday, April 26, 2012 at 10:46pm by krystal

Chemistry
For a. You have 0.00 mL of NaOH; therefore the pH will be determined solely by HCl. pH = -log(0.250) pH = 0.602
Saturday, April 27, 2013 at 3:02am by DrBob222

Ph CHEM
It is; however, your calculation gives you pOH. If you want pH, use pH + pOH = pKw = 14 and solve for pH. Or you can use (H^+)(OH^-) = Kw = 1E-14 pH = -log(H^+) pOH = - log(OH^-)
Tuesday, November 27, 2012 at 9:31pm by DrBob222

special ed
Another thought -- Unless you were teaching extremely low functioning students, vacuuming and dusting would not be appropriate for high schoolers. I urge you to spend several hours in various special ed classrooms for the mentally impaired.
Saturday, September 26, 2009 at 11:39am by Ms. Sue

investing
How do I find stock on margin rate of return? This is the question: Ed Delahanty purchased 500 shares of Niagara Corporation stock on margin at the beginning of the year for $30 per share. The initial margin requirement was 55%. Ed paid 13% interest on the margin loan and ...
Wednesday, July 23, 2008 at 6:53pm by Anonymous

chem101
OH^- = 7.76E-9 (H^+)(OH^-) = Kw = 1E-14 Solve for H^+, then convert to pH [pH = -log(H^+)] and see if it is within the brackets set between 5.5 and 5.9 for pH.
Friday, November 30, 2012 at 1:35am by DrBob222

Chem 1A
Help please! How many moles of NaOH must be added to 1.0 L of 3.0 M HC2H3O2 to produce a solution buffered at each pH? 1) pH= 3.78 2) PH= 6.52
Thursday, March 15, 2012 at 10:01pm by Mackenzie

Chemistry
This just adds to the information provided by Bob Pursley. pH<7 = acid pH=7 = neutral pH>7 = basic (alkaline)
Monday, August 22, 2011 at 1:00pm by DrBob222

Chemistry
The formula is pH=pKa+log([A-]/[HA]) A- is the base, HA is the acid. So, Before titration HCl+H2O->H3O+ + Cl- pH=-log[H30+] pH=-log(.100) b/c HCl is a strong acid, it equals [H30+] pH=1 At equivalence point, pH=7
Monday, March 18, 2013 at 8:24pm by Kaylin

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