A solution in water has 1.0x10E-5 moles of H+ ion in 10.0 liters of solution. -What is the pH? -What is the concentration of the OH- ion? My notes give an example of: 3.75 x 10E-4 with the result of -3.425968732 However, when I attempt to run the example through my calculator I end up with 0.60205999...
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)  NaCl (aq) + H2O (l) Problem 10.85 What are the [H3O+] and [OH-] for a solution with the following
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
Consider the following titrations: a. 50.0 mL of 0.100 M HClO4 titrated by .0500 M KOH b. 60 mL of 0.400 M HF titrated by 0.800 M RbOH For each of the titrations, determine the pH: i. Initially, before any titrant has been added ii. At the halfway point to equivalence iii. At the equivalence point.
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
What mass of acetic acid (CH3CO2H) is required to generate 10.0L of 50.0 mM acetic acid solution?
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
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
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
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
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. )
What are the formulas for: lead(II) carbonate copper(II) Cyanide And chemical formula for slaked lime
The first step in the Oswald process for producing nitric acid is: 4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g) If the reaction of 150 g of ammonia with 150 g of oxygen gas yields 87g of nitric oxide(NO), what is the percent yield of this reaction?
Oxalic acid H2C2O4 is a diprotic acid. Calculate the mass of acid in a solid given that a 0.7984 g sample of that solid required 45.00 mL of 0.300 M NaOH for neutralization.
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. 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. 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
Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 e -6. Its unionized form is red and its anionic form is yellow. What color would a methyl red solution have a pH = 7.8? red yellow blue violet green For this problem I am confused on how to start... Can you please help me?
You are given a vial of unknown monoprotic weak acid. You weigh out .5000g of the acid and dissolve it in pure water to make a final volume of 100 ml. Your instructor requires you to use the entire 100.0 ml of acid solution in a single titration trial. In this trial, it takes 27.24 ml of .1500 M NaOH to reach the equivalence poi
In a buffer solution, a constant solution pH is maintained regardless of the amount of acid or base added. True or False?
A certain aqueous solution contains 6.0 e -6 moles of dissolved KSCN. This solution occupies a total volume 50.0 ml. What is the concentration of SCN-?
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?
What are pH, [H3O+], [HSO3-], and [SO32-] in a 1.50 M sulfurous acid 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?
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.
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.
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.
Benzoic acid (C6H5COOH) is sometimes used as a standard to determine the heat capacity of a bomb calorimeter. When 1.44 g C6H5COOH is burned in a calorimeter that is being calibrated, the temperature rises from 19.18 degrees Celsius to 22.93 degrees Celsius. What is the heat capacity of the calorimeter? The heat of combustio
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
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