Monday

April 21, 2014

April 21, 2014

Number of results: 91,440

**math**

d = your digit d = 100 x + 10 y + z my hundreds digit is three more than my ones x = z + 3 that is equivalent with : z = x - 3 my tens digit is oneless than my hundreds y = x - 1 d = 100 x + 10 y + z d = 100 * x + 10 * ( x - 1 ) + x - 3 d = 100 x + 10 x - 10 + x - 3 = 111 x - ...
*Thursday, August 16, 2012 at 5:30am by Bosnian*

**ALGEBRA**

A chemist is asked to make 10 liters of a a35% solution. She has only a 10% solution and a 50% solution to work with. how much of each solution must she mix to ge 10 liters of the 35% solution?
*Saturday, January 28, 2012 at 4:23pm by jackie*

**chemistry**

Which solutions are acidic? (Assume all solutions are at 25°C. Kw = 1.0 x 10-14 at 25°C.) A. A solution with [H+] = 9.4 x 10-6 B. A solution with [H+] = 5.5 x 10-10 C. A solution with pH = 6.1 D. A solution with [OH-] = 6.4 x 10-7 E. A solution with [OH-] = 2.0 x 10-6
*Friday, October 8, 2010 at 11:53am by Ceci*

**Chemistry**

What is the H+ ion concentration of this solution? A solution is made by dissolving 0.0112 g KOH in enough water to make 1.0 liter of solution. What is the H+ ion concentration of this solution? a. ) 2.0 x 10-3 M b. ) 8.0 x 10-2 M c. ) 1.2 x 10-13 M d. ) 5.0 x 10-11 M e. ) 5.0...
*Saturday, November 1, 2008 at 11:46pm by Joey22*

**Chemistry**

What is the H+ ion concentration of this solution? A solution is made by dissolving 0.0112 g KOH in enough water to make 1.0 liter of solution. What is the H+ ion concentration of this solution? a. ) 2.0 x 10-3 M b. ) 8.0 x 10-2 M c. ) 1.2 x 10-13 M d. ) 5.0 x 10-11 M e. ) 5.0...
*Monday, November 3, 2008 at 10:59pm by Angelo09*

**CHEIMISTRY**

A buffer solution is 0.20 M in HPO42- ions and 0.l0 M in H2PO4- ions. What is the H3O+ ion concentration of the solution? The ionization constants for H3PO4 are as follows: Ka1 = 7.5 ´ 10 -3, Ka2 = 6.2 ´ 10-8, Ka3 = 1 ´ 10-12. a. 3.7 ´ 10-3 M b. 3.7 ´ 10-4 M c. 3.1 ´ 10-8 M d...
*Sunday, May 30, 2010 at 2:27pm by james*

**Science**

5. You have made the following two solutions: X) hydrogen ion concentration = 1 x 10-5M Y) pH = 4 State which statements below are true and which are false: a. Solution X contains 1 x 10-9M hydroxide ions. b. Solution X contains more H+ ions than Solution Y. c. Solution Y ...
*Monday, September 10, 2012 at 1:03pm by Alex*

**Chemistry**

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 ´ 10^-4 M. What is the equilibrium constant, Ka, for this acid? a. 5.0 ´ 10^-2 b. 5.0 ´ 10^-3 c. 2.5 ´ 10^-4 d. 2.5 ´ 10^-5 e. 2.5 ´ 10^-6 2. (Points: 1) What is the carbonate-ion, CO3^-2, ...
*Thursday, May 13, 2010 at 7:34am by write2khin*

**Chemistry**

0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 * 10^-4 M. What is the equilibrium constant, Ka, for this acid? a. 5.0 *10^-2 b. 5.0 * 10^-3 c. 2.5 * 10^-4 d. 2.5 * 10^-5 e. 2.5 * 10^-6 2. (Points: 1) What is the carbonate-ion, CO3^-2, ...
*Thursday, May 13, 2010 at 5:26pm by wite2khin*

**chemistry**

For a 10 w/v% solution, we want 10 g solute in 100 mL solution. To obtain 10 g HCl from 37% solution, we need to take 10/(0.37*1.19) = 22.7 g of the concd solution. (Check: 22.7 mL x 1.19 g/mL x 0.37 = 10 grams.) Make the final volume to 100 mL and you will have 10 g/100 mL ...
*Monday, June 22, 2009 at 5:10am by DrBob222*

**chemistry**

The concentration of HNO3 in a solution is 3.50 10-6 M. What is the [H3O+] in the solution? _______M What is the [OH-] in the solution? ________ M What is the pH of the solution? What is the pOH of the solution?
*Tuesday, December 21, 2010 at 8:26pm by jim*

**pharmacy tech.**

Prepare 500ml of a 1:5 solution using a 1:10 solution and a 1:4 solution. What quantities will be used of each stock solution to make the 1:5 solution?
*Sunday, August 5, 2012 at 6:59pm by blackpearl07*

**chemistry**

The concentration of NaOH in a solution is 7.00 10-6 M. What is the [H3O+] in the solution? _______________M What is the [OH-] in the solution? __________M What is the pH of the solution? What is the pOH of the solution? HELPP?? i don't understand any of this...
*Wednesday, December 22, 2010 at 4:17pm by jim*

**pharmacy calculations**

prepare 500 ml of a 1:5 solution using a 1:10 solution and a 1:4n solution. what quantities will be used of each stock solution to make the 1:5 solution?
*Friday, August 3, 2012 at 1:08pm by cleondra*

**algebra**

I answered your post below with this same question. Please check to see if your post was answered before re-posting. I pasted the answer here for you. x = liters of 3% solution 3 - x = liters of 10% solution .03x = value 3% solution .10(3 - x) = value 10% solution 3 = liters ...
*Sunday, January 23, 2011 at 11:23pm by helper*

**chem**

232 ppm = 232 g Cl^-/10^6 g solution = 232 x 10^-6 g Cl^-/g solution. Since the solution is so dilute, the density of the solution will be essentially 1.00 g/mL; therefore, this is equivalent to 232 x 10^-6 g Cl^-/mL or for a liter it is 232 x 10^-6 x (1000 mL/1L) = 232 x 10^-...
*Thursday, February 12, 2009 at 11:45pm by DrBob222*

**Chemistry**

Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below, followed by the pH of ...
*Tuesday, May 27, 2008 at 7:38pm by Tom*

**Science/Chem**

1. You dissolve 157.1 g of ammonium nitrate in a 250 mL volumetric flask and add water to the mark (call this solution A). You take 30 mL of solution A and place it in a 100 mL volumetric flask and add water to the mark (this is solution B). Next you take 50 mL of solution B ...
*Sunday, September 28, 2008 at 4:40pm by Kelsey*

**science/chem**

You dissolve 157.1 g of ammonium nitrate in a 250 mL volumetric flask and add water to the mark (call this solution A). You take 30 mL of solution A and place it in a 100 mL volumetric flask and add water to the mark (this is solution B). Next you take 50 mL of solution B and ...
*Sunday, September 28, 2008 at 4:41pm by Kelsey*

**Chem**

Please tell me if these are right! What are the [H3O+] and [OH-] for a solution with the following pH values? a. 10.0 I got 1.0*10^-10 for [H3O+] and 1.0*10^-4 for [OH-] b. 5.0 I got 1.0*10^-5 for [H3O+] and 1.0*10^-9 for [OH-] c. 7.00 I got 1.0*10^-7 for [H3O+] and1.0*10^-7 ...
*Wednesday, December 8, 2010 at 1:34pm by Jessica*

**Chemistry**

Assignment Calculate the pH, pOH, [H+], and [OH] for each of the following solutions. Show all work. (10 Points) Solution Composition of Starting Materials 1 0.10 M acetic acid 2. 5 mL 0.10 M acetic acid + 5 mL wa 3 1 mL 0.10 M acetic acid + 99 mL water 4 5 mL...
*Monday, October 11, 2010 at 12:24pm by Brian*

**Chemistry 2**

A saturated solution of a certain metal(II) chloride has a chloride ion concentration of 0.032M. The Ksp for this compound can be determined to be a) 2.6 X 10-7 b) 4.1 X 10-6 c) 1.6 X 10-5 d) 2.6 X 10-4 e) 1.6 X 10-2 I am unsure how to approach this problem or the steps to ...
*Thursday, April 5, 2012 at 8:55am by Sheri*

**chem**

1. What is the [K+] of a solution prepared by dissolving 0.140 g of potassium hydroxide in sufficient pure water to prepare 250.0 ml of solution? 2. What is the pH of a 0.570 M solution of aniline? Kb = 7.4 × 10-10
*Monday, March 31, 2008 at 7:43am by nelson*

**Chemistry**

Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL 3.0e-4M bromescol green solution 25.0mL 1.60M ...
*Monday, October 29, 2012 at 1:48pm by Jake*

**Chem.**

Can you also check this one, Please and thank-you! 23. Acetylsalicylic acid, commonly known as ASA, is the most widely used drug in the world. ASA has the chemical formula, C8H7O2COOH, and a Ka of 3.27 X 10 – 4 mol/L. What is the pH of a 10 mol/L ASA solution? The pH of the ...
*Wednesday, July 19, 2006 at 11:07pm by Jacy*

**chemistry**

A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp? Is the solution unsaturated, saturated, or supersaturated? Will a precipitate form in ...
*Monday, April 23, 2012 at 12:35am by Anonymous*

**chemistry**

A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp? Is the solution unsaturated, saturated, or supersaturated? Will a precipitate form in ...
*Tuesday, April 24, 2012 at 9:52am by Anonymous*

**chemistry**

A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp? Is the solution unsaturated, saturated, or supersaturated? Will a precipitate form in ...
*Tuesday, May 8, 2012 at 1:55pm by Anonymous*

**Chemistry **

A solution of PbI2 has [Pb2+] = 4.5 x 10-5 and [I-] = 6.5 x 10-4. PbI2 has Ksp = 8.7 x 10-9. Write down the reaction that is taking place. Calculate Q. Is Q larger or smaller than the Ksp? Is the solution unsaturated, saturated, or supersaturated? Will a precipitate form in ...
*Tuesday, May 8, 2012 at 6:00pm by Vanessa*

**math again**

How does "How many gallons of a 12% indicator solution must be mixed with a 20% indicator solution to get 10 gal of a 14% solution?" turn into ".12x + .2(10+ -1x) = .14(10)"?? Please, I need to understand how it works! Thank you.
*Sunday, February 22, 2009 at 8:44am by James*

**Chemistry**

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution. (potentially useful info: Ka of NH4+ = 5.6 x 10−10)
*Wednesday, July 17, 2013 at 1:55am by Nat*

**Math help!**

1.(g + 4) - 3g = 1 + g 1 4 No solution Identity 2. 5y + 2 = 1/2(10y + 4) 5 10 No solution Identity 3. 0.5b + 4 = 2(b + 2) 0 0.5 No solution Identity 4. -3x + 5 = -3x + 10 5/6 -5/6 No solution Identity My answers: 1. 1 2. Identity 3. 0 ??? Not sure 4. No solution I really need ...
*Tuesday, October 1, 2013 at 7:08pm by Charlotte*

**Chemistry help!!!**

Calculate [H3o+] in each aqueous solution at 25*C, and classify each solution as acidic or basic. a. [OH-]= 1.1 x 10^-9M b. [OH-]= 2.9 x 10^-2M c. [OH-]= 6.9 x 10^-12M
*Monday, March 14, 2011 at 4:38pm by sally*

**Chemistry**

A solution that contains 2.047 x 10^-1 M of acid, HA, and 1.808 x 10^-1 M of its conjugate base, A-, has a pH of 4.196. What is the pH after 1.629 x 10^-3 mol NaOH is added to 5.961 x 10^-1 L of this solution?
*Saturday, January 21, 2012 at 11:17pm by Summer*

**Chemistry**

How do the following solutions show the properties of a buffer? 1) 50 ml 0.10 M NH3 + 50 ml 0.10 M NH4NO3 2) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M HCl 3) 10 ml solution #1 + 6 ml 0.10 M HCl 4) 10 ml solution #1 + 5 ml H2O + 1 ml 0.10 M NaOH
*Wednesday, March 20, 2013 at 2:27pm by Jeremy*

**Please Help CHEM**

Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the ...
*Tuesday, December 7, 2010 at 2:03pm by Jessica*

**Chemistry**

What volume of a .500 M HCl solution is needed to neutralize each of the following: 10 ml of a .300 M NaOH solution 10 mL of a .200 M Ba(OH)2 solution
*Tuesday, March 8, 2011 at 3:13am by Monty*

**chemistry**

A solution contains 1.72 10-3 M Ca(NO3)2. Determine the mass of the Ca2+ ions in 1.8 mL of this solution. How many nitrate ions are there in 3.0 10-6 L (3.0 µL) of this solution? (i keep doing these two wrong but not sure why)
*Tuesday, April 24, 2012 at 11:31pm by katiy*

**General Chemistry**

find [H3O+] and [OH-] 1)a solution that is 5.8×10−2 M in [HBr] and 1.9×10−2M in [NO3]. 2)a solution that is 0.780% HNO3 by mass (Assume a density of 1.01 g/mL for the solution.)
*Wednesday, October 10, 2012 at 11:41am by jv*

**Help Chemistry**

Can you please tell me if these are right? Determine the pH for the following solutions A [OH-] = 1.0 X 10^-7 M I got 7 B. [H3O+ = 4.2 X 10 ^-3M I got 2.4 C. [H3O+]= 0.0001M I got 4 D. [OH-] = 8.5 X10^-9M I got 5.9 What are the [H3O+] and [OH-] for a solution with the ...
*Tuesday, December 7, 2010 at 11:01am by Jessica*

**Chemistry**

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 ´ 10-4 M. What is the equilibrium constant, Ka, for this acid? a. 5.0 ´ 10-2 b. 5.0 ´ 10-3 c. 2.5 ´ 10-4 d. 2.5 ´ 10-5 e. 2.5 ´ 10-6 2. (Points: 1) What is the carbonate-ion, CO3-2, ...
*Thursday, May 13, 2010 at 7:34am by write2khin*

**Chemistry. PLEASE HELP**

a) To make an acid solution, 6.8 x 10-3 mole of a strong acid (6.8 x 10-3 mole H3O+) is dissolved in water to give a 550 mL solution. What is the pH and [OH-] of the solution? b) 150 mL of water is added to 50 mL of the solution produced in question 3. Calculate the new pH of ...
*Thursday, October 17, 2013 at 9:37am by Anonymous*

**Chemistry**

a) To make an acid solution, 6.8 x 10-3 mole of a strong acid (6.8 x 10-3 mole H3O+) is dissolved in water to give a 550 mL solution. What is the pH and [OH-] of the solution? b) 150 mL of water is added to 50 mL of the solution produced in question 3. Calculate the new pH of ...
*Thursday, October 17, 2013 at 2:02am by Anonymous*

**Chemistry**

I have a 40 ml solution of pH 4.36. I need to make this solution at pH 8.5 by adding extra 10 ml of HCl and NaOH. Not sure that this question entirley makes sense. However, if pH is 4.36 then pOH is 9.74 and [OH-] is 1.82 x 10^-10 M if target pOH is 5.5 then [OH-] is 3.16 x 10...
*Monday, August 6, 2012 at 7:49am by DrRuss*

**algebra**

a chemist needs 10 liters of a 25% acid solution. the solution is to be mixed from three solutions whose acid concentrations are 10% 20% 50% how may liters of each solution should the chmist use to satisfy the following? a use as little as possible of the 50% solution b use as...
*Saturday, April 26, 2008 at 8:21pm by sandy*

**microbiology**

This is an inverse proportion problem: 5*10^8*1 = 1*10^3*V V=5*10^8 / (1*10^3) =5*10^5 times the initial volume. So the dilution is 1 ml of the initial solution and 5*10^5-1 = 499999 litres diluent (water?) to make a total volume of 500000 ml, or 500 litres of diluted "solution".
*Sunday, May 8, 2011 at 8:16pm by MathMate*

**Chemistry**

A) Determine the pH of a 0.98 x 10^-2 mol L solution of hydrocyanic acid (HCN) Ka = 4.0 x 10^-10 B) What is the pH of a 0.243mol L solution of methylamine? (pKb for CH3NH2 = 3.30) C) determine the pH of a buffer solution of Na2CO3 (pkb = 3.68, 0.125 M) and NaHco3 (0.35M)
*Monday, June 3, 2013 at 10:07pm by Jake*

**Chemistry**

Solution x has a pH of 4.35. Solution y has 10- times high [OH-] compared to solution x. Solution z has a pH 4.0 units higher than that of solution x. calculate the ration of [H3O+] between solutions x&y and between x&z. What is the pH of solutions y and z? classify each ...
*Tuesday, March 19, 2013 at 2:12pm by mary*

**Chemistry**

I may have missed something but I believe this needs rethinking. As I read the problem, the final solution concn is 10 ng/mL (and not 10 ng/10 ml). I assume this is 10 ng/mL in the 10 mL methanol solution. Then 10 ng/mL x 10 mL = 100 ng in the final 10 mL methanol soln. That ...
*Friday, January 11, 2013 at 2:50pm by DrBob222*

**Chemistry**

A solution is 0.10M Pb(NO3)2 and 0.10M AgNO3. If solid NaCl is added to the solution what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10^-5; AgCl = 1.8 x 10^-10) The answers is 1.4 x 10^-8 How do I find the answer
*Sunday, October 14, 2012 at 6:07pm by Fred*

**Math help**

1. Which value is a solution of the equation 5 - 4x = -3 0 2 -3 1/4 2. Which ordered pair is a solution of the equation y = x - 4 (2, 6) (6, 2) (-2, 6) (3, -1) 3. Which ordered pair is a solution of the equation y = 3x (-2, -9) (-8, -18) (-8, -3) (-10, -30) 4. Which ordered ...
*Tuesday, October 15, 2013 at 6:58pm by Charlotte*

**Chemistry Acid/bases**

The concentration of H2SO4 in a solution is 3.20 10-6 M. Assume the acid dissociates completely in solution. What is the [H3O+] in the solution? What is the [OH-] in the solution? What is the pH of the solution? What is the pOH of the solution? OK SO I KNOW HOW TO DO THESE ...
*Tuesday, February 10, 2009 at 8:11pm by Spencer*

**math**

a pharmacist mixed some 10% saline solution with some 15% saline solution to obtain 100ml of a 12%saline solution.How much of 10% saline solution did the pharmist use in the mixture.dO NOT UNDERSTAND TO MUCH INFO.
*Thursday, May 6, 2010 at 7:58pm by Anonymous*

**chem**

if a 10cm cube pipette were not available, which one of the following would be the best way of measuring a 10cm cube portion of a solution? a. weigh 10 times the mass of 1cm cube of the solution. b. weigh 10g of the solution. I think this is a trick question. There seems to be...
*Friday, December 22, 2006 at 4:18am by minerva*

**Math**

Theoretically they need 90ml & 3% = 2.7ml of 100% solution. Let x=volume of 10% solution, then 90-x = volume of 1% solution. x*10% + (90-x)*1% = 2.7 Multiply by 100: 10x + (90-x) = 270 Solve for x and check. I get 20ml 10% and (90-20)ml 1%.
*Sunday, December 5, 2010 at 10:05pm by MathMate*

**Chemistry**

(Ksp= 5.0*10^-13) 1) Calculate the molar solubility of AgBr in 3.0×10^−2 M AgNO3 solution. 2) calculate the molar solubility of AgBr in 0.10 M NaBr solution. I tried solving using this the quadratic formula, but it didn't work. I started with these equations and then ...
*Sunday, March 17, 2013 at 9:33pm by Jonah*

**College Chemistry**

What is the pH of the following solutions? 1)a solution that is 5.4×10−2 M in HClO4 and 3.0×10−2 M in HCl 2)a solution that is 1.80% HCl by mass (Assume a density of 1.01g/mL for the solution.) Please help! I am so confused!
*Sunday, March 7, 2010 at 4:49pm by Katie*

**Math**

A druggist mixes a 10% solution of iodine with a 15% solution of iodine. How much of each solution should be used in order to obtain 20 cubic centimeters of a 12% solution?
*Wednesday, February 10, 2010 at 11:02am by Vinnnie*

**chemistry**

You have a 10 M acidic solution. However, you need that solution to be 0.25 M. How many ml of 10 M should be diluted to obtain 300 ml of 0.25 M acid solution?
*Sunday, October 24, 2010 at 3:53pm by gerg*

**chemistry**

You have a 10 M acidic solution. However, you need that solution to be 0.25 M. How many ml of 10 M should be diluted to obtain 300 ml of 0.25 M acid solution?
*Monday, January 3, 2011 at 4:42pm by markees*

**Chemistry**

To make an acid solution, 6.8 x 10-3 mole of a strong acid (6.8 x 10-3 mole H3O+) is dissolved in water to give a 550 mL solution. What is the pH and [OH-] of the solution?
*Thursday, October 17, 2013 at 1:07am by Anonymous*

**Math**

If a mixture of a 6% acid solution with an 11% solution is to be made, how much of each solution is needed to make 10 liters of an 8% acid solution?
*Sunday, September 2, 2012 at 9:40am by DAD*

**math**

A 10% acid solution is to be mixed with a 50% solution to get 200 liters of a 20% solution. How many liters of each solution should be used?
*Sunday, June 23, 2013 at 8:42pm by Monica*

**math**

60 ml of solution A is mixed with 120 ml of solution B to produce solution C which contains 8% of pure acid. If 80ml of solution A is mixed with 40ml of solution B, a solution D containing 10% of pure acid can be produced. find the percentage of pure acid in solution A?
*Tuesday, July 5, 2011 at 2:18am by anjan*

**math**

60 ml of solution A is mixed with 120 ml of solution B to produce solution C which contains 8% of pure acid. If 80ml of solution A is mixed with 40ml of solution B, a solution D containing 10% of pure acid can be produced. find the percentage of pure acid in solution A?
*Tuesday, July 5, 2011 at 2:18am by anjan*

**chemistry**

A 1.0 L solution has 10.00 grams of CaCl2 dissolved in it. What is the Molar solubility of AgCl in this same solution? The Ksp for AgCl is 1.6 x 10-10 at this temperature. Hint: watch out for the common ion again.
*Saturday, April 12, 2014 at 11:18am by bekah*

**algebra**

looks very similar to the question just posted by Lily. let the amount of 30% solution we want to add be x l now let's reason it through.... the volume of acid we have before adding is .3(10) l or 3 l we are adding x l of a 20% solution so we are adding .2x l but the final ...
*Monday, July 21, 2008 at 12:51pm by Reiny*

**chemistry**

1. Find the pH of a solution whose [H3O+] is 9.5 X 10^ -8 M. 2. What is the [H3O+] concentration of a solution with a pH of 5.45? 3. What is the pOH of a solution with a [OH -] concentration of 2.97 X 10^ -10 M?
*Monday, May 14, 2012 at 12:41pm by kellin*

**chemistry**

Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship. The combination is the pH of Solution A described below, followed by the pH of ...
*Tuesday, May 27, 2008 at 9:36pm by Tom*

**math**

A lab needs a 20 liters of a 15% acid solution. The lab only has a 10% acid solution and a 30% acid solution. How much of the 10% acid solution will they need to mix with the 30% solution to obtain 20 liters of a 15% solution?
*Tuesday, April 2, 2013 at 5:42pm by Anonymous*

**Chemistry**

Consider a solution containing 4.35 mM of an analyte, X, and 1.09 mM of a standard, S. Upon chromatographic separation of the solution peak areas for X and S are 3251 and 10075, respectively. Determine the response factor for X relative to S. F=? To determine the concentration...
*Friday, June 7, 2013 at 5:06pm by ScienceGeek*

**chemistry**

find the pH of 10 mL of 1.00M solution after adding 10.00mL of indicator solution
*Monday, February 14, 2011 at 7:08pm by Anonymous*

**science**

You have 10 ml of a 1:10,000 solution of hydrogen peroxide (H2O2). What is the molar concentration of the solution?
*Monday, September 5, 2011 at 1:58pm by Marcus*

**urgent chem help ( dr bob plz)**

A particular household ammonia solution (d= 0.97g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 650 mL of a solution with pH = 11.55? ------------------------- i am gettig 5.3 x 10^-10 is tht rite or worng pzl conform ..
*Tuesday, February 17, 2009 at 9:44pm by javeya*

**algebra**

x = liters of 3% solution 3 - x = liters of 10% solution .03x = value 3% solution .10(3 - x) = value 10% solution 3 = liters of 7.9% mixture .079(3) = 0.237 = value 7.9% mixture .03x + .10(3 - x) = 0.237 Solve for x, which is number of liters of 3% solution. (3 - x) = number ...
*Sunday, January 23, 2011 at 10:37pm by helper*

**math**

A nurse needs to make 30 ml of 5% solution of glucose. She has available bottles containing 5 ml of 7% solution and bottles containing 10 ml of 1% solution. How many 5 ml bottles and 10 ml bottles will she need to make the solution? Bottles of 5 ml of 7% solution needed: ...
*Monday, March 11, 2013 at 8:40pm by Josh*

**algebra**

If the value is a solution then it will make the statement true when it is substituted in. 3*2+4=10 10 is grater then 9 so 2 is a solution. To get a number that makes this false we can solve 3x+4=9. X=5/3
*Monday, February 14, 2011 at 6:02pm by Johnathon*

**Chemistry**

A 7.2 ´ 10-3 M solution of acetic acid is 5.0% dissociated. In a 7.2 ´ 10-4 M solution, the percentage of dissociation would be a. the same. b. >5%. c. <5%. d. zero. e. none of these
*Thursday, May 26, 2011 at 2:22am by Roxanne*

**chemistry**

A solution has H+ = 5.0 ´ 10–5 M. Assume temperature of the solution is 25 Centigrade.The pH of this solution is?
*Tuesday, June 12, 2012 at 10:07pm by sidd*

**chemistry**

a saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.5. What is the hydronium concentration of the solution? is the solution acidic or basic?
*Tuesday, July 14, 2009 at 7:10pm by angela*

**Chem**

A solution is prepared by adding of KOH to 1 liter of water. The resulting solution has an [OH] of 1*10 to the negative 3. What would be the pOH of this solution?
*Thursday, April 28, 2011 at 12:44am by Carla M*

**Chemistry - help please**

In an experiment, when 25 mL of 5.5 x 10^-3 M NaOH is mixed with 30 mL of 7.5 x 10^-3 M Fe(Br)2, a hydroxide compound is formed (Ksp = 1.8 x 10^15). Which of the following describes the resulting solution? a. The product is unsaturated b. The mixture product is saturated c. ...
*Tuesday, October 15, 2013 at 12:05pm by Eren*

**chemistry**

Indicate whether each solution is acidic, basic, or neutral. a. [H3O+] = 6.9 x 10-1 M This solution is acidic. b. [H3O+] = 8.2 x 10-13 M This solution is basic. c. [H3O+] = 3.2 x 10-1 M This solution is acidic.
*Monday, February 27, 2012 at 4:42pm by krystal*

**chemistry**

ndicate whether each solution is acidic, basic, or neutral. a. [H3O+] = 6.9 x 10-1 M This solution is acidic. b. [H3O+] = 8.2 x 10-13 M This solution is basic. c. [H3O+] = 3.2 x 10-1 M This solution is acidic.
*Wednesday, February 29, 2012 at 12:26am by krystal*

**chemistry**

A 10% acid solution is to be mixed with a 50% acid solution in order to get 120 ounces of 20% acid solution. How many ounces of the 10% solution and 50% solution should be mixed?
*Monday, April 26, 2010 at 6:52pm by Meliss*

**Chemistry**

What is the pH of a solution containing 0.10 M propanoic acid (HC3H5O2) and 0.10 M sodium propanoate after 0.02 mol of HCl is added to 1.0 L of the solution?
*Sunday, February 28, 2010 at 8:39pm by Blake*

**algebra **

Please help!!! Determine whether -10 is a solution of the equation 6(x-2)= -70 Is -10 a solution? Thanks for your help
*Monday, November 8, 2010 at 6:41pm by thawk*

**algebra 2**

How much of an 18% solution of sulfuric acid should be added to 360 ml of a 10% solution to obtain a 15% solution?
*Tuesday, June 22, 2010 at 11:07am by Derron*

**Chemistry**

Calculate the amount of solute needed to make each of the solution: 225g of 10% (m/m) K2CO3 solution .50kg of a 18% (m/m) KOH solution
*Friday, May 13, 2011 at 5:58pm by Curlyqty*

**chem101**

If a solution contains 0.0100 mole of HCl in 10.0 mL aqueous solution. a.) What is its molarity? My answer is 1M (0.0100 mole/10.0 mL * 1000 mL/1L = 1M) b.) What is H^+ ion concentration for this solution? c.) What is the expected pH for this solution? pls help i don't know ...
*Wednesday, November 28, 2012 at 9:32am by audrey12*

**chemistry**

A particular solution has a [H3O+] 2.44 x 10^-4. Therefore, the [OH-]= 4.10 x 10^3 4.10 x 10^-11 2.44 x 10^-4 1.71 x 10^-8 9.09 x 10^-16
*Monday, December 5, 2011 at 2:45pm by Anonymous*

**chemistry**

Use algebra to solve the quadratic equation 1.7*10^-5 *(c - 0.02) = 4*10^-4 c^2 which can be rewritten 4*10^-4 c^2- 1.7*10^-5 c +3.4*10^-7 = 0 c^2 -4.25*10-2 c + 8.5*10^-4 = 0 It appears there is no real-number solution to this equation, because B^2 - 4AC is negative. (A, B ...
*Saturday, February 14, 2009 at 3:35pm by drwls*

**Math**

How do you solve for this:how many gallons of a 10% alcohol solution be mixed with 20 gallons of a 10% acid solution to obtain an 8% acid solution.
*Sunday, May 30, 2010 at 11:14pm by krystal*

**Chemistry**

10% (m/m) Sodium Hydroxide solution, NaOH(aq) is used to break down wood fibre to make paper. A) What mass of the solute is needed to make 250mL of 10% (m/m) solution? B) What mass of solvent is needed? C) What is the molar concentration of the solution?
*Monday, May 2, 2011 at 9:28am by Saman*

**math**

in the lab, tom has two solutions that contain alcohol and is mixing them with each other. he uses 300 millilters less of solution A than solution B. solution A is 10% alcohol and solution B is 13% alcohol. How many millilters of solution B does he use, if the resulting ...
*Thursday, September 27, 2012 at 12:31pm by Anonymous*

**chemistry**

a lab experiment calls for 10% acetic acid solution. The lab has only 5% and 15% acetic solutions available. How much of each should be mixed to obtain 10 liters of a 10% solution?
*Thursday, December 1, 2011 at 7:46pm by Brandy*

**Math**

determine weather 10 is the solution of the equation x+10=36 is 10 the solution no use multiplcation principle 10x=-90 -9 3[7-9{6-2)]= -87 find -x when x=-62/83*= 62/83
*Sunday, November 8, 2009 at 10:25pm by Conrad*

**Math**

determine weather 10 is the solution of the equation x+10=36 is 10 the solution no use multiplcation principle 10x=-90 -9 3[7-9{6-2)]= -87 find -x when x=-62/83*= 62/83
*Sunday, November 8, 2009 at 11:03pm by Conrad*

**Math**

determine weather 10 is the solution of the equation x+10=36 is 10 the solution no use multiplcation principle 10x=-90 -9 3[7-9{6-2)]= -87 find -x when x=-62/83*= 62/83
*Sunday, November 8, 2009 at 11:41pm by Conrad*

**Chemistry**

Calculate the equilibrium concentration of all ionic aqueous species in a solution containing 1.30 M HCl and 4.0 M C6H5OH (phenol, Ka=1.6 x 10^-10). What is the pH of the solution?
*Saturday, April 19, 2008 at 12:29am by Gloria*

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