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# Acids and Bases

### Concentration, titration, pH and pOH of solutions.

Please see the attached file for the fully formatted problems. Problem 10.53 What is the molarity of an HCl solution if 11.0 mL HCl solution is titrated with 21.6 mL of 0.130M NaOH solution? HCl (aq) + NaOH (aq) &#61664; NaCl (aq) + H2O (l) Problem 10.85 What are the [H3O+] and [OH-] for a solution with the following

### Solutions : Acids, bases, Salts, pH and Concentration

Label each of the following as an acid, base or salt, explaining your answer: a. KOH b. HCl c. Ba(OH)2 d. H3PO4 e. FeSO4 2. Calculate the pH of the following solutions with the given [H+] or [OH-] and indicate whether it is an acid or base: a. [OH-] = 0.01 b. [H+] = 0.001 c. [OH-] = 0.0

### buffer solution challenged by HCl

I have four problems that I don't understand how to figure out. I've done problems 16-20 but don't know how to do 21-24. I've attached the whole page from the exam for the information it provides. I've boxed my previous answers in case they are needed to figure out the four questions. I need help on the third page. The secon

### Use Henderson-Hasselbalch to explain how buffers work.

Fully explain the following two questions: 1. Using the Henderson-Hasselbalch equation, or other appropriate equations, discuss why the optimum pH with a respect to a buffer's ability to act as a buffer is within ± 1 pH unit of the buffers pKa. 2. Does the ocean have a buffer system in place? How is the pH of the ocean

### Estimation of pH of solution based on color of 2 indicators

Please see the attached file for the fully formatted problems. 1. Estimate the pH of the following, based on the indicator colors given: Solution Tested Bromocresol Green (indicator color) Bromothymol Blue (indicator color) Estimated pH Distilled water Blue Yellow

### Solutions : Molarity; understanding acid-base titrations and balanced equations, C1V1=C2V2

I am confused on how to calculate the concentratin of the HCl solution - below are the answers so far that I have to get the final answer -please help. I am stumped on question 2 The concentration of the NaOH is known to be 0.1M 1. For your most exact titration, record the following: (a) Volume of NaOH solution in

### How to write a chemistry lab report

A full lab report, including propagation of error, with instructions on what belongs in each section (abstract, introduction, experimental, results and discussion, acknowledgments, references, and appendices). This sample lab concerns the determination of the percent chloride in a soluble unknown, but has general notes for each

### equilibrium pressure of HOCl

Questiom 12 The equilibrium constant Kp = 0.90 for the following reaction in the gas phase: H2O(g) + Cl2O(g) 2HOCl(g). Calculate the equilibrium pressure of HOCl in the reaction vessel if the initial pressures of H2O and Cl2O are both 0.35 atm. show work a. ) 0.11 atm. b. ) 0.18 atm. c. ) 0.22 atm. d. )

### Using indicators to measure acidity

Please help with the following multiple choice questions regarding acids and bases. You have two neutral solutions. One contains the indicator methyl red, which turns red in strongly acidic aqueous solutions but is otherwise yellow. The other contains the indicator phenol red, which turns red in strongly basic aqueous soluti

### A 55-year-old woman visits a popular eatery for lunch.

A 55-year-old woman visits a popular eatery for lunch. She orders a cheese and bacon pizza with extra cheese and has about 3 large glasses of cola (ph value 3). On the way back home, she experiences heartburn and abdominal pain, and has difficulty breathing. She drinks a lot of water and has to consume milk of magnesia (pH value

### A 40-year-old manager, at a prominent legal firm in L.A., experiences abdominal pain post lunch. ...

A 40-year-old manager, at a prominent legal firm in L.A., experiences abdominal pain post lunch. He goes to the restroom a couple of times, but continues to experience pain and cramps. He eventually decides to get himself examined. While questioning him, you learn that he consumed two bottles of beer at lunch. The alcohol (ethyl

### pH of individual blood

Need help with these attached questions. 1. If an individual has a HCO3- = 23 mmol/L and PCO2 = 48 mmHg, what is the pH? 2. if an individual has a pH = 7.55 and a PCO2 = 39 mmHg, what is the concentration of HCO3-? 3. if an individual has a pH = 7.40 and a HCO3- = 18 mmol/L, what is the partial pressure of PCO2?

### 35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the final solution?

35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the final solution?

### Groundwater Dissolved Oxygen

Please show how to solve this problem. A ground water sample , at 25 C, has Eh= 1.0 and pH=6.80. Assuming the system is at equilibrium, calculate the amount of dissolved oxygen (ppm) in the groundwater sample.

### PH of Co2 saturated water

Please show how to solve. Calculate the pH of CO2-saturated water at 25 degrees C, given that the CO2 concentration in air is 338 and that for carbon dioxide the Henry's Law constant KH=3.4E-2 mol L-1 atm-1 at 25 degrees C. Furthermore, the ionization constant, Ka, for H2CO3 has a value of 4.5E-7 mol L-1 at this temperature.

### Concentration of Atmospheric CO2

If the concentration of atmospheric CO2 were to double from its current value of 330 ppm, what would be the calculated pH of rainwater assuming that CO2 was the only acidic input? Please show step by step.

### Questions Regarding Equilibrium Reactions

1. Given the following reaction H2(g) + I2 (s) = 2HI (g) ¤h = + 68.0 KJ/mol A) Write the Kc expression. B) State whether the number of moles of H2 (g) in the container will increase, decrease, or remain the same after each of the following disturbances is applied to the original mixture. For each case, assume that al

### pH and Ka of lactic acid

3. Lactic acid, HC3H5O3, is a monoprotic acid that dissociates in aqueous solution, as represented by the equation(not given). Lactic acid is 1.66 % dissociated in 0.50M HC3H5O3. (aq) at 298K. A) Write the expression for the acid- dissociation constant , Ka , for lactic acid and calculate its value. B) Calculate the pH

### Relative Strong of Conjugate Base

17. Using the following Ka values , indicate the correct order of of the conjugate base strength HNO2. Ka = 4.0 x 10-4 HF. Ka = 7.2 x 10 -4 HCN. Ka = 6.2 x 10-10 A. CN- > NO2- > F- > H2O > CL- B. CL- > H2O > F- > NO2- > CN- C. CN- > F- > NO2- > CL- > H2O D. H2O > CN- > NO2- > F- > CL- E. None of the ab

### properties of HF and the strongest base in the reaction

5. When comparing 0.050M HF (aq) and 0.010M HF (aq) which of the following statements is false ? A. The pH of 0.050M is lower than the pH of 0.01M B. The percent ionization of 0.010M is greater than 0.050M C. The electrical conductivity of 0.050M is greater than 0.010M D. All of the above ( therefore the statements are

### The Enthapy Change of a Chemical Reation involving Mg

Lab Tools : Thermometer, Balance Lab Glassware : Calorimeter Lab Chemicals : H2O, Mg, HCl Lab Background : When an exothermic reaction takes place in a container, heat is released and warms up the container and its contents. The contents of the container include the reaction products and a solvent (such as water), if

### Acids, Bases, Titrations and Indicators

4) Aniline, a weak base, reacts with water according to the reaction represented above. a) Write the equilibrium constant expression, Kb, for the reaction represented above. b) A sample of aniline is dissolved in water to produce 25.0mL of a 0.10M solution. The pH of the solution is 8.82. Calculate the equilibrium constsant

### pH of solution

Weak acid - strong base 50.0ml of 0.20 M HCOOH ( Ka = 1.8 x 10^-4) with 0.1 M NaOH A) what volume of NaOH will be added at equilibrium ? B) what is the initial pH ? C) between initial and equivalence point D) at equivalence point E) beyond equivalence point F) what happens exactly halfway to the equivalence po

### buffered solution

Short answer: A) pH of a buffer is determined by : B) buffer capacity is determined by :

### pH of Buffer Solution: Sodium Lactate and Lactic Acid

1) A buffer is prepared by adding 0.200 mol of sodium lactate ( NaC3H5O3) to 500ml of 0.5 M lactic acid ( Ka = 1.4 x 10^-4). A) What is the pH of the buffered solution? B) What is the pH after 100ml of 0.100 M HCL is added to the buffer? C) What is the pH after 12 g of NaOH is added to the original solution prepared in

### titration of hypochlorous acid using NaOH

5) Ka = [H3O+ ] [OCL ]. = 3.2 x 10^-8 ................................. [HOCL ] Hypochlorous acid , HOCl , is a weak acid in water with the above Ka A) write a chemical equation showing how HOCl behaves as an acid in water B) calculate the pH of a 0.175 M solution of HOCl C) write the

### pH of the solution

4). calculate the pH of a 0.265 M solution of propanoic acid HC3H5O2 (aq) = C3H5O2- (aq) + H+ (aq), Ka = 1.34 x 10^-5 Propanoic acid ionizes in water according to the equation above A) write the equilibrium- constant expression for the reaction B) calculate the pH of a 0.265 M solution of propanoic acid 5) A 0.496

### Dissociation of HF in Water and Reaction with Strong Base

1. HF(aq) + H2O(l) <----> H3O+(aq) + F- (aq) Hydrofluoric acid dissociates in water as represented by the above equation With Ka = 7.2 * 10^-4 A) write the equilibrium- constant expression for the dissociation of HF(aq) in water B) calculate the molar concentration of H3O+ in a 0.4M HF solution HF reacts with NaOHaq ac

### Draw the structure of the dye formed from Primuline red and 2-naphthol.

1) Discuss the results of your classification tests and melting point of your derivatives. What is your unknown? How do your data exclude other possibilities and what, if anything is still inconsistent with your conclusion? "Boiling Point for the Unknown is 218oC. For the 2,4-dinitrophenylhydrazone derivative of the unknown, th

### Neutralization of Acetic Acid with NaOH

Write a balanced equation for the neutralization of acetic acid with NaOH. I have actually gotten better at balancing equations---but I have no idea where to even start with this one. Any help you can provide would be greatly appreciated. Thank You,