Q: 1 A student dilutes a 0.25 M HCI solution to obtain a 0.025M solution. The student then measures the…
A: Concentration of the diluted HCl solution = 0.025 M Measured pH of the diluted HCl solution = 1.75…
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A: Kb is the dissociation constant of a weak base. Higher is its value, stronger is the base.
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A: pH= -log[H+] Using this formula [H+] can be calculated.
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A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
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Q: Part A Calculate the pH of a solution that is 0.260 M in sodium formate (HCOONa) and 0.090 M in…
A: here is the solution
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A: Since you have posted a question with multiple sub-parts we will solve the first three for you. To…
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A: Due to common ion effect extent of dissociation of a substance decreases. NaCl is strong…
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A: Given, pH = 8 PH is defined as negative logarithm of concentration of [H+] ion.
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Q: 37. A solution has a pH of 10.65. What is the [H3O+] value for this solution?\ a. 2.2 x 10-11 b. 4.5…
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A: Since, you have asked multiple questions then I solved step by step first question for you. You can…
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A: Given :- concentration of HNO3 Solution = 0.174 M To calculate :- pH of solution
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A: At 25 oC, the solubility of barium hydroxide, Ba(OH)2 is approximately 4.70 g / 100 mL water. Since…
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A: Acid and bases are different chemicals, which have some certain characteristics. By measuring pH, we…
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A: given equation, HClO4(aq) + H2O(l)→ ClO4-(aq) + H3O+(aq) HClO4 is a strong acid with initial…
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A: Given : Mass of Ba(OH)2 = 601 mg = 0.601 g…
Q: determine the concentration of the base.
A: Molarity = number of moles/volume of solution (in L) Number of moles = molarity × volume(in L)
Q: 24. Calculate the pH of each of the following strong acid solutions. (a) 0.00831 M HI pH =_____ (b)…
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
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Q: 36. Determine the pH of 0.25 M HBr solution. * A. 0.30 B. 0.52 C. 0.60 O D. 13.0
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A: Ammonia is a weak base, it is a Lewis base.
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A: pH is defined as the negetive logarithm of Hydrogen ion concentration. That is, pH = -log[H+]
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A: pH is used to determine the concentration of hydronium ion.
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A: pH is used to determine the concentration of hydronium ion.
Q: Ph a b доби 24 Ph Ph 25 27 CI ОН НО CI 26 28
A:
Q: 93. Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is K for…
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- A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?Find [H+] and the pH of the following solutions. (a) A 456-mL sample of a 12.0% (by mass) solution of HNO3(d=1.00g/mL). What is the pH of 10.0 mL of the same sample? (b) A solution made up of 1.0 g of HCI dissolved in enough water to make 1.28 L of solution. What is the pH of the solution? If the same mass of HCI is dissolved in enough water to make 128 mL of solution, what would the pH be?Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
- A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
- For an aqueous solution of acetic acid to be called distilled white vinegar it must contain 5.0% acetic acid by mass. A solution with a density of 1.05 g/mL has a pH of 2.95. Can the solution be called distilled white vinegar?For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.A solution of KOH has a pH of 13.29. It requires 27.66 mL of 0.2500 M HCI to reach the equivalence point. (a) What is the volume of the KOH solution? (b) What is the pH at the equivalence point? (c) What is [K+] and [Cl-] at the equivalence point? Assume volumes are additive.
- Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxideConsider two weak acids, HA (MM=138g/mol)and HB (MM=72.0g/mol). A solution consisting of 11.0 g of HA in 745 mL has the same pH as a solution made up of 5.00 g of HB in 525 mL. Which of the two acids is stronger? Justify your answer by an appropriate calculation.Use the same symbols as in Question 61 ( = anion, =OH) for the box below. (a) Fill in a similar box (representing one liter of the same solution) after 2 mol of H+ (2) have been added. Indicate whether the resulting solution is an acid, base, or buffer. (b) Follow the directions of part (a) for the resulting solution after 2 mol of OH- (2 ) have been added. (c) Follow the directions of part (a) for the resulting solution after 5 mol of OH- (5 ) have been added. (Hint: Write the equation for the reaction before you draw the results.)