What is the pH of a .0078M solution of KOH? Choices: 1. 2.2 2. -2.2 3. -11.9 4. 11.9
What is pH of a .0045M HCl solution. Choices: 1.2.3 2.-2.3 3.11.6 4.-11.6
Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work) 1. Write the equation: 2. What is the pH of the solution before titration begin
You have an unknown organic compound that is soluble in acetic acid. If 39.35g of this compound in 29.95ml of acetic acid (density of acetic acid is 1.0492g/mL) has a freezing point of 8.650 degrees Celsius, what is the molar mass of this organic compound? The freezing point of acetic acid is 16.60 degrees Celsius and the fre
Which ion(s) is/are spectator ions in the formation of a precipitate of AgBr via combining aqueous solutions of CoBr2 and AgNO3? a. Co2+ and Ag+ b. Co2+ and NO3- c. NO3- and Br- d. NO3- e. Br- Which of the following is an exchange reaction? a. 2SO(g) + O2(g) ---> 2SO2(g) b. CaCO3(s) ---> CaO(s) + CO2(g) c. F
Calculate the pH upon diluting 2ml of 2 N HCL to a final volume of 100 ml? Calcuate the pH upon addition of 0.0075 mole of solid NaOH to 100 ml of a 0.1 M solution of acetic acid (pKa=4.7)? If equal molar amounts of Na2HPO4 and NaJpo4 are mixed in water, calcuate the resulting pH. The pKas of phosphoric acid are 2.1, 7.2,
-------------------------------------------------------------------------------- Do you feel inclined to think that titration of acid and base at equivalence point will always yield a neutral solution? Well the answer is no. Learn from the following excersie. Weak Acid - Strong Base Titration. a 50.0-mL portion of 0.200
Please help with the ones marked red. (See problem set in attached file).
A 50.0-mL portion of 0.200 M HCOOH is titrated with 35.0 mL of 0.200 M KOH. What is the pH after this titration is complete?
Preparing a Buffer. The pH of blood is 7.40. Calculate the [HCO3-] / [H2CO3] ratio of a bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40. Hint: the Henderson-Hasselbalch equation is useful for this type of problem.
A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?
What is the pH of a solution that contains 0.250-M benzoic acid and 0.600-M sodium benzoate?
Hello, I am trying to find out how to plug in to calculator, to solve for PH, POH and others by using what was given. Hope I provided more information this time
Which of the following cannot act as a Lewis base? A. Cl- B. NH3 C. BF3 D. H2O
A 0.200 M aqueous solution of HI has a pH of _____ @ 25 C?
Calculate the concentrations of hydrogen ion and hydroxide ion at 25 degrees C. 1. Aniline, C6H5NH2, is used in the manufacturing of some perfumes. What are the values for a 0.035 M solution? Kb= 4.2 x 10-10 [H+]= [HO-]= 2. For a solution in which 10.0 mL of 0.100 M HCl is added to 25.0 mL of 0.100 M NaOH [
1. A buffer was prepared from equal molar quantities of acetic acid, HC2H3O2 and sodium acetate, NaC2H3O2. Explain how the buffer keeps the pH of the solution at about the same value (a) after the addition of a few drops of a dilute HCl solution and (b) after the addition of a few drops of a dilute NaOH solution. Use reaction eq
1. Will the solution formed by dissolving each of the following salts in water be basic, neutral or acidic? Write the equation to show how each ion of each salt affects the PH of the solution. 1. Na3PO4 2. NH4Cl 3. CH3COONa Please show each step in detail.
Please provide assistance with the following questions: 1. Processed cheese must be at a pH of 5.5 to 5.9 to prevent the growth of unwanted microorganisms. The quality control supervisor receives a report that a sample has a [OH-] of 1.2x10^-8. Find pH, pOH, [H+] of this sample. 2. How many grams of potassium hydroxide,
Please can you help me, I need to find balanced chemical equations for: a) The reaction of calcium phosphide and water to produce phosphine and calcium hydroxide; b) The oxide formed when phosphorus burns in air, dissolves in water to give a solution of phosphoric acid (H3PO4).
I have a selection of apparatus and materials that I could use to prepare a gas jar of dry phosphine. I have the following pieces of apparatus to use:- Wash bottle Polythene connectors Dropping funnel with rubber stopper Bent glass tube Filter funnel with paper U-tube Porcelain boat Gas jar Round bottomed flask w
In chemistry, I am not sure what "pkw" stands for.
What is the pH of 0.50-M sodium benzoate? The benzoate ion (C7H5O2-) is the anion of benzoic acid.
Sodium bicarbonate was added to an unlimited amount of sulfuric acid undergoing a reaction to produce sodium sulfate plus carbonic acid (which turned in to water vapor and carbon dioxide upon heating). Please provide a balanced equation for this reaction.
1. Write a balanced equation for the reaction of calcium phosphide with water to produce phosphine and calcium hydroxide, in a atmosphere of carbon dioxide at 0C and a pressure of 4.8mm Hg. At STP carbon dioxide has a density of 1.96g/litre, and phosphine has a density of 1.53g/litre. Liquid water is used in the reaction. 2.
The following acid-base reaction is performed in a coffee cup calorimeter: H+(aq) + OH-(aq) --> H2O(l) The temperature of 110 g of water rises from 25.0°C to 26.2°C when 0.10 mol of H+ is reacted with 0.10 mol of OH-. * Calculate qwater * Calculate ΔH for the reaction * Calculate ΔH if 1.00 mol
Observations: 1) A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2. 2) B does not react with any of the 1mol/L solutions above or the dilute sulfuric acid. 3) C reacts spontaneously with dilute sulfuric acid and with 1mol/L solutions of all the other metallic
Could you please explain what happens when hydrogen ions are added to a mixture of barium chromate (S) and chromate ions (AQ). Would there be a precipitate and, if not, why?
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 + 2.5E10-6. In order to make up a buffer solution of pH 5.80, which combination would you choose, NaHA/H2A or Na2A/NaHa? What is pKa of the acid component? I don't understand this problem at all! I know that a diprotic substance has something i
I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer. The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I ca