A 25 mL sample of .175 M CH3NH2 is titrated wiht .160 M HBr. What is the volume of the equivalence point.

Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.

Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.

Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?

What acid-base indicators, shown in Figure 18.24 would be suitable for the neutralization reaction whose titration curve is shown in Figure 18.30?Why?

Rust, which you can take to be Fe(OH)3, can be dissolved by treating it with oxalic acid. An acid-base reaction occurs, and a complex ion is formed. (a) Write a balanced equation for the reaction. (b) What volume of 0.10 M H2C2O4 would be required to remove a rust stain weighing 1.0 g?

Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.

1) A 45 mL sample of 0.175 M KOH is titrated with 0.200 M HI. a. b. c. d. Find the initial pH of the 0.175 M KOH solution. Find the pH when 18 mL of 0.200 M HI have been added. Find the pH when 63 mL of 0.200 M HI have been added. How many milliliters of 0.200 M HI must be added to reach the equivalence point? e. What is the pH at the equivalence point? f. Draw a titration curve for this titration. g. Which of the following indicators should be used to signal the endpoint of this titration: methyl red (pK₁ = 5.5), litimus (pK₁ = 7.0), or phenolphthalein (pK, = 8.7)? Explain.

A sample of pure diprotic acid required 45.50 mL of 0.2000M NAOH to reach the second equivalence point. Given that the molar mass of the acid is 126.1 g/mol, determine the weight (in grams) of the sample that was titrated. Oo.5738 Oo.2868 O1.1475 Omore information is required

3. The titration of a 20.0-mL sample of an H₂SO₄ solution of unknown concentration requires 22.87 mL of a 0.158 M KOH solution to reach the equivalence point. What is the concentration of the unknown H₂SO₄ solution?