A 0.5130 g aspirin tablet which was dissolved in 95 percent ethanol required 27.98 mL of 0.1000 M NaOH for neutralization. Then an additional 42.78 mL of 0.1000 M NaOH was added and the soln was heated to hydrolyze the

28,677 results

chemistry

A 0.5130 g aspirin tablet which was dissolved in 95 percent ethanol required 27.98 mL of 0.1000 M NaOH for neutralization. Then an additional 42.78 mL of 0.1000 M NaOH was added and the soln was heated to hydrolyze the aceytlsalicyclic acid. After the reaction mixture was ...

Chemistry

Acetylsalicylic acid (C9H8O4) is a monoprotic acid commonly known as "aspirin." A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took 12.25 mL of...

General Chemistry

A 0.179 g sample of a vitamin C tablet was titrated with 0.1000 M NaOH according to the procedure in this experiment. The titration required 7.08 mL of NaOH solution. How many moles of NaOH were used in the titration?

Chemistry

3) A student dissolves a 1.18g aspirin tablet in water and titrates the solution with a .265M NaOH. 22.05mL of NaOH are required to reach the equivalence point. Calculate the percentage of acetylsalicylic acid in the tablet.

Chemistry

A 0.179 g sample of a vitamin C tablet was titrated with 0.1000 M NaOH according to the procedure in this experiment. The titration required 7.08 mL of NaOH solution. How many moles of NaOH were used in the titration? How Many moles of Vitamin C were in the sample? What was ...

College Chemistry

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

chem

quantitative determination of acetylsalicylic acid in aspirin tablets by back titration 1)why do we use a more dilute NaOH solution for the standardization of NaOH? 2)what is the rationale behind the dilution and aliquoting of the aspirin sample? 3)what are the principles ...

Chemistry

A certain headache relief tablet is composed of monoprotic acetylsalicylic acid(C9H8O4(s)) and an inert filler. A 4.00 g tablet was crushed and dissolved to make 40.0 mL of solution. The solution was then titrated with 0.900 mol/L NaOH(aq). The volume of NaOH(aq) needed to ...

chemistry

I need some help with calculating percent yield and percent purity of aspirin. Here's my data (questions follow): SYNTHESIS Mass of salicylic acid.., 2.0 g Volume of acetic anhydride.., 5 mL Mass of watch glass.., 22.10 g Mass of aspirin and watch glass.., 28.01 g Mass of ...

Chemistry

Mass of an aspirin tablet is 0.42g and contains 77.38% ASA by mass. I dissolved the tablet in hot naOH and cooled the solution with distilled water to the mark of 250 volumetric flask. Then I pipetted 5.0 mL of the solution to the 100 mL volumetric flask and I diluted it with ...

chemistry

An aspirin tablet weighing 0.548 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

CHEM 102

Can someone help me with this question please? What is the pH at each of the points in the titration of 25.00 mL of 0.1000 MHCl by 0.1000 M NaOH:i) After adding 25.00 mL NaOH ii) After adding 26.00 mL NaOH thankyou

CHEM 102

Can someone help me with this question please? What is the pH at each of the points in the titration of 25.00 mL of 0.1000 MHCl by 0.1000 M NaOH:i) After adding 25.00 mL NaOH ii) After adding 26.00 mL NaOH thankyou

College-Chemistry

NaOH(s)+ H2SO4(aq)=Na2SO4(aq) + H2O(l) Consider the unbalanced equation above.A 0.900 g sample of impure NaOH was dissolved in water and required 37.0 mL of 0.145 M H2SO4 solution to react with the NaOH in the sample. What was the mass percent of NaOH in the sample?

chemistry

A student dissolves a .726 g aspirin tablet in water and titrates the solution with .272 M NaOH are required to reach the equivalence point. Calculate the percentage of acetylsaliclic acid in the tablet. I am not really sure where to start with this. I unfamiliar with problems...

Chemistry II

A 12.00 mL sample of sulfuric acid from an automobile battery requires 34.62 mL of 2.42 M sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? H2SO4 + 2NaOH ==> Na2SO4 + 2H2O molarity NaOH x liters NaOH = mols NaOH. mols H2SO4 = ...

chem

I titrated a 250mg tablet to see if it really had 250mg of scorbutic acid (H2C6O6) a diuretic acid, in it. I took a 250mg tablet, grounded it up and found it took 35.87ml of .0505 M NaOH to neutralize it 1. How many moles of NaOH is it? 35.87ml NaOh(1L/1000ml) (.0505M/1L)= ....

Chemistry

What volume of 0.1000 M oxalic acid (a diprotic acid) would be required to completely neutralize 100.00 mL of 0.1000 M NaOH?

Chemistry

What volume of 0.1000 M oxalic acid (a diprotic acid) would be required to completely neutralize 100.00 mL of 0.1000 M NaOH?

chemistry

4g NaOH is dissolved in 100mL of 2.5M H2SO4 will be required for its complete neutralization?

Chemistry

A 0.2800 g sample of an unknown acid requires 28.22 mL of 0.1199 M NaOH for neutralization to a phenolphthalein point. a.) How many moles of OH- are used? b.) How many moles of H+ are found in the acid? c.) What is the calculated equivalent molar mass of the unknown acid? If I...

chemistry- pH, neutralization

What volume of NaOH was required to have neutralized the HCl. HCl + NaOH --> H2O + NaCl There no other information given in the problem except in later questions like the NaOH had 0.1 M and that there was 50.00 mL of HCl.

Chemistry

Antacid tab is dissolved in water and a few drops of phenolphthalein is added yielding bright pink solution. 0.2025 M HCl added until pink color disappears. The 0.2147 M NaOH added until it turns light pink for ~30 seconds. mass on antacid tablet = 1.056g initial V 0.2025 M ...

science

C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in water to make 100ml of ...

chemistry

A sample of carboxylic acid is added to 50.0 mL of 2.27 M NaOH and the excess NaOH required 28.7 mL of 1.86 M HCl for neutralization. How many moles of NaOH reacted with the carboxylic acid?

chemistry

A TUMS tablet was dissolved in 110.00 ml of 0.1022 M HCl and analyzed for CaCO3 according to the procedure described in the lab manual. It took 7.48 ml of 0.1005 M NaOH to reach the endpoint. Calculate the mass of CaCO3 in TUMS tablet to the correct number of significant ...

Chemistry

10. For the titration of 20.00 mL 0.1000 M lactic acid with 0.1000 M NaOH, calculate the pH: a. before any titrant is added b. 10.00 mL prior to the equivalent point c. at the equivalent point d. 10.00 mL after the equivalence point. Plot the points obtained on a graph of pH ...

Chem 1212

An antacid tablet containing calcium carbonate as an active ingredient required 9.19 mL of 0.0956 M H2SO4 for complete neutralization. The mass of the tablet was 0.193 g. What percent of calcium carbonate was in the tablet? Thanks!

chemistry

What is the mass percent of a solution if 42.9 grams of aspirin is dissolved into 175 mL of ethanol? (Density of ethanol is 0.789 g/mL

chemistry

What is the mass percent of a solution if 42.9 grams of aspirin is dissolved into 175 mL of ethanol? (Density of ethanol is 0.789 g/mL) 1. 31.1 % 2. 24.5 % 3. 23.7 % 4. 19.7 %

Chemistry

A sample of 8.44 grams of NaOH is dissolved into 536 mL of aqueous 0.250 M NaOH (assume no volume change). This solution is then poured into 1.96 gallons of water. You may assume that the two volumes can be added.) What is the concentration of NaOH in the final solution? ...

college chem

What would the [OH-] be after addition of 17.47 mL of 0.1000 M NaOH to 25.00 mL of 0.1000 HA (a weak acid, Ka = 3.16e-4)?

chemistry

Describe in detail how you would prepare 1000 ml of 0.1 M NaOH from 6 M of NaOH stock solution.

chemistry

A student performs a back-titration to determine the cost -effectiveness of an antacid. A tablet with a retail cost of $0.053 is dissolved in 25.00 ml of 1.000 M HCl, then back-titrated with 1.000 M NaOH. Exactly 14.82 ml of NaOH solution is required to reach the endpoint. ...

chemistry

An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

chemistry

An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

chem

An aspirin tablet weighing 0.650 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

chemistry

An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

Chem.

An aspirin tablet weighing 0.400 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

Chemistry

An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

chemistry

Mass of Aspirin tablet: 0.357 g 10 mL of 1 M NaOH was added to the aspirin tablet in a 125 mL Erlenmeyer flask and heated to a boil. The solution was transferred to a 100 mL volumetric flask and the flask was filled to the mark with DI water. 1 mL of the solution was pipetted ...

college chemistry

An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

science

the teacher instructed three students A,B,and C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in water to make 100ml of ...

science

the teacher instructed three students A,B,and C respectively to prepare a 50% (mass by volume) solution of sodium hydroxide (NaOH). 'A' dissolved 50 g of NaOH in 100 ml of water B dissolved 50g of NaOH in 100g of water while C dissolved 50g of NaOH in water to make 100ml of ...

Chemistry

Calculate the pH during the titration of 40 ml of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: A.) 28.00 ML B.) 39.80 ML C.) 48.00 ML

chemistry 101

If 15g of NaOh is dissolved in 285 g of water, calculate the following. Assume the density of the solution is 1.06 g/cc. a) Calculate the moles of NaOH in the solution? My answer is 15gNaOH/40g NaOH= .0375 mole NaOH b) Waht is the mass % w/w of the solution? My answer is 15g ...

Chemistry

I dissolved 4g of solid NaOH in 200mL of water. I converted grams of NaOH to moles by 4g/40g/moles= 0.1moles. I calculated the concentration of NaOH by 0.1/(200mL/1000L)= 0.5 moles/L. I now have to record the expected mass of benzoic acid required to react in stoichiometric ...

chemistry

Find the pH during the titration of a 20.00mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka=1.54 x10^-5), with the addition of 10 mL of 0.1000 M NaOH solution??

Chemistry

An antacid tablet weighing 1.462 grams was dissolbed in 25mL of 0.8M HCl and diluted with water. The excess HCl was titrated with 3.5 mL of 1.019M NaOH solution. 1. Calculate the number of millimoles added to the tablet 2. Calculate the number of millimoles of NaOH required to...

Chemistry

An antacid tablet weighing 1.462 grams was dissolbed in 25mL of 0.8M HCl and diluted with water. The excess HCl was titrated with 3.5 mL of 1.019M NaOH solution. 1. Calculate the number of millimoles added to the tablet 2. Calculate the number of millimoles of NaOH required to...

chemistry

1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH ...

chemistry

A 0.205 g sample of impure NaOH requires 17.5 mL of 0.2180 M HCl for neutralization. What is the percent of NaOH in the sample, by weight?

chemistry

Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3CH2CH2COOH with 0.1000 M NaOH after 26.5 mL of the base have been added. Ka of butanoic acid = 1.54 x 10-5.

chemistry

Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3CH2CH2COOH with 0.1000 M NaOH after 26.5 mL of the base have been added. Ka of butanoic acid = 1.54 x 10-5.

chem

An aspirin tablet weighing 0.650 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

Chemistry

Exactly 23.6 ml of a 0.131 N HCl solution was required for complete neutralization of 25.0 ml of an NaOH solution.What was normality of the NaOH?

biology

suppose 23mL of NaOH was required. How much Carbonic Acid was neutralized? 1L of .01 NaOH contains ____ mol NaOH? lmL of .01 NaOH contains _____mol NaOH? 23mL of .01 NaOH contains _____ mol NaOH? 2 mol of NaOH react with 1 mol H2CO3 2.3 x 10^-4 mol of NaOH react with ____mol CO2

chem

An aspirin tablet weighing 0.475 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL of the solution was ...

Chemistry

Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka = 1.54e-5), with 0.1000 M NaOH solution after the following additions of titrant: 0 mL, 14.00 mL, 19.95 mL, 20.00 mL, 20.05 mL, 24.00 mL.

college chemistry

A 0.300 g sample of an aspirin tablet is used to prepare 100.0 mL of a stock solution by dissolving the tablet in 1 M NaOH then diluting with distilled water to the 100 mL mark of a volumetric flask. A 0.30 mL sample of the stock solution is then transferred to a volumetric ...

Chemistry

A 1.250 g mass of standard aspirin is dissolved in approximately 20 mL of 1 M NaOH. This solution is added to a 250-mL volumetric flask and diluted to the mark with DI water. How many grams per mL of aspirin are in the resulting solution? (Note that a 250-mL volumetric flask ...

College Chemistry

Calculate the Molarity of the solution that contains 4.00 grams of NaOH in a total volume of 1500.0 mL. [Molar Mass NaOH = 40.00g, 1 Liter = 1000 mL]

Chemistry

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

Chemistry

Neutralization reaction HCL(aq) + NaOH(aq) -> NaCl(s) + H2O(l) Use your results to determine the netball change of the neutralization reaction, in kJ/mol of NaOH, Write the thermochemical equation for the neutralization reaction. I'm not sure how to even go about doing this...

Chemistry

Hi,may I have your help? I have posted a titration question that I'm trying to solve. The correct answer to the problem is 0.128 M, however,I have arrived at the answer: 0.000128 M. Here's the question: If 38.30 mL of 0.250 M NaOH is used to titrate 25.0 mL of phosphoric acid,...

chemistry

A 3.664 g sample of monoprotic acid was dissolved in water and required 20.27 mL of a 0.1578 M NaOH solution for neutralization . Calculate the molar mass of the acid

Chemistry

For the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaoH, calculate (a) the initial pH; (b) the pH when neutralization is 50% complete; (c) the pH when neutralization is 100% complete; and (d) the pH when 1.00 mL of NaOH is added beyond the equivalence point.

chemisrty

A 21.00 sample of 0.3254M Hcl solution requires 26.09 ml of NaOH solution for complete neutralization. Calculate the volume of NaOH solution in liters, required for the titration.

Inorganic Chemistry

I messed up on my titration: filled part of the burette with a supersaturated solution of KHTar(2.073g...MM=188.18amu) dissolved in 150mL diH2O, instead of the 0.051M NaOH solution. I know it wasn't more than a few mL, but I noticed a huge difference in the volume of NaOH ...

CHEMISTRY

ANTACID TABLET OF WEIGHT 1.3183G WAS DISSOLVED IN 75 MLOF CONC. HCl OF 0.1807M IS TITRATED WITH 20.36ML OF CONC. NaOH OF 0.1481M . FIND MILIMOLES OF HCl ADDED, FIND MILIMOLES OF NaOH USED IN TITRATION, FIND MILIMOLES OF HCl THAT DID NOT REACT WITH ANTACID, FIND MILIMOLES OF ...

Chemistry

44.70 ml of 0.100 M NaOH are required to completely neutralize 50.00 ml of a weak monoprotic acid, HA. When 34.43 ml of NaOH are added to another 50.00 ml of the acid, the pH reading was 4.80. Calculate Ka for the acid using the partial neutralization method.

chem

Sulfuric acid reacts with sodium hydroxide according to this equation: H2S04 + 2 NaOH Na2(SO4) + 2 H2O A 10.00 mL sample of the H2SO4 solution required 13.71 mL of 0.309 M NaOH for neutralization. Calculate the molarity of the acid.

Chemistry

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

Chemistry

An impure sample of (COOH)2 · 2 H2O that has a mass of 2.9 g was dissolved in water and titrated with standard NaOH solution. The titration required 32.4 mL of 0.144 mo- lar NaOH solution. Calculate the percent (COOH)2 · 2 H2O in the sample.

CHEMISTY

A 25.0 mL sample of perchloric acid solution required 45.3 mL of 0.101 sodium hydroxide solution for complete neutralization. what was the concentration of the perchloric acide solution? work: 0.0453 L NaOH x ( .101 mol NaOH/ 1L NaOH) x (1 mol HClO4/ 1 mol NaOH) x (25.0 mL ...

Chemistry: Molarity

4.82 mL of a 0.262 M NaOH solution reacts completly with 4.79 mL of HCl solution according to the balanced chemical reaction shown below: HCl (aq) + NaOH (aq) -> NaCl*aq) + H2O (I) What is the molarity of the HCl solution? 4.82 x (1L/1000 mL) = .00482L 4.79 x (1L/1000 mL...

Chemistry

Which of these is true about the following reaction? NaOH + HCl ¡æ NaCl + H2O A. NaOH is the proton acceptor. B. HCl acts as the Br©ªnsted-Lowry acid. C. NaOH and HCl are the products. D. This is an example of a neutralization reaction. E. The products will be acidic. Okay...

chem

An impure sample of (COOH)2 ·2 H2O that has a mass of 3.4 g was dissolved in water and titrated with standard NaOH solution. The titration required 42.7 mL of 0.156 molar NaOH solution. Calculate the percent (COOH)2 · 2 H2O in the sample. Answer in units of %.

Chemistry

How do I solve these problems You have 2000. g of aqueous NaOH solution. The percent by mass of the solute is 4.25%. How many grams of NaOH are in the solution? If you have 100.0 mL of a 25.0% aqueous solution of ethanol, what volumes of ethanol and water are in the solution?

chemistry

If 58g of NaOH are dissolved in water to make a final volume of exactly 400mL, what is the molar concentration of NaOH? (The FM of NaOH = 40.0) How do I set this up?

chem

In the following balanced neutralization reaction equation, how many moles of HCl are required to completely neutralize 0.040 moles of NaOH? HCl + NaOH d NaCl + H2O

rhs

n the following balanced neutralization reaction equation, how many moles of HCl are required to completely neutralize 0.040 moles of NaOH? HCl + NaOH → NaCl + H2O

CHEMISTRY

200.0 ml of 0.5000 M acetic acid is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid at 25 oC is 1.76 x 10-5. n(NH3COOH)=CxV=0.5x200/1000=0.1mol n(Naoh)=CxV=0.5x200/1000=0.1mol I have no idear of what to do after finding the number of moles

Chemistry-Is this correct?

The concentration of NaOH is normally in the range of 3-6 M when they peel potatoes and soak them in a solution of NaOH , remove them and spray them off. If I have 45.7 mL of 0.500M of H2SO4 required to react completely with a 20.0 mL sample of NaOh. What is the molar ...

math

1.64g of a mixture of cac03 and mhco3 was dissolved in 50ml of 0.8M hcl. The excess of acid required 16ml of 0.25M naoh for neutralization. Calculate the percentage of cac03 and mgc03 in the sample Who helps me

Chemistry

In this experiment NaOH is standardized to titrate it with vinegar so thtat the percent by mass of the acetic acid can be determined. How does dissolved CO2 in distilled water affect the accuracy of the determination of a NaOH solution's concentration? How is the term acid ...

Math

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

Chemistry

One commercial method used to peel potatoes is to soak them in a solution of NaOH for a short time, remove them from the NaOH, and spray off the peel. The concentration of NaOH is normally in the range of 3 to 6 M. The NaOH is analyzed periodically. In one such analysis, 45.7 ...

chemistry (AP)

The heat of neutralization of HCl (aq) by NaOH is -55.9Kj/mol H2) produced. If 50ml of 1.6M NaOH at 25.15 celsius is added to 25ml of 1.79M HCl at 26.34 celsius in a plastic foam cup calorimeter, what will be solution temperature be immediately after the neutralization ...

Chemistry

A 0.1873 g sample of a pure, solid acid, H2X was dissolved in water and titrated with 0.1052 M NaOH solution. The balanced equation for the neutralization reaction occurring is H2X(aq) + 2NaOH(aq) ¨ Na2X(aq) + 2H2O(l) If the molar mass of H2X is 85.00 g/mol, calculate the ...

chemistry

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

Chemistry

Why is the heat of neutralization between HCL and NaOH is higher than CH3COOH and NaOH

Chem

Why should a dilute NaOH solution be used for the standardization of NaOH in the analysis of Aspirin using back titration?

chem

how to find mass of aspirin if I used 0.2845g of the powder(crushed apririn) with 1mL of 6.0 mol/L of Nacl? Does the dilution(the above chemicals are diluted in a 500mL volumetric flask) matter ,and does adding the HCL/Fe^3+ stock solution in the end matter (1.00 mL of the the...

Chemistry

An antacid tablet containing magnesium hydroxide instead of calcium carbonate was dissolved in 100.0 mL of 0.2893 M HCL. 10 mL of this solutions was titrated to endpoint with 25.20 mL of 0.1007 M NaOH. How much magnesium hydroxide was in the antacid tablet(in mg)? Any help is ...

chemistry

If 5.30mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00 mL of 0.1000 M HCl was added to 1.00 g of an antacid, how many moles of acid can the antacid counteract per gram?

Math

Find the amount of money in the account at the end. $1000.00, 4 years, 7% compounded semi-annually A=P(1+r/n)^nt r=0.07, t=4, P=$1000.00, n=2 A=P(1+r/n)^nt A=$1000.00(1+0.07/2)^2-4 A=$1000(1.035)^8 A=$1000(1.316809037) A=$1,316.809037 My answer is: A=$1316.81 is this right?

CHEMISTRY

Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the NaOH?

CHEMISTRY

Suppose a student adds 25.00 mL of 1.025 M HCl to a 1.50 g antacid tablet. The student boils and then titrates the resulting solution to the endpoint with 0.4969 M NaOH. The titration requires 21.3 mL NaOH to reach the endpoint. How many moles of HCl were neutralized by the NaOH?

Chemistry

Calculate the pH of the the solution that results from titrating 50 mL of 0.6 M HCN(aq) with 0.2 M NaOH At 0.00 mL of NaOH At 85 mL of NaOH. At 150 mL NaOH. At 160 mL of NaOH

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