HF is a weak acid (a monoprotic one). When HF is titrated with a strong base...
HF is a weak acid (a monoprotic one). When HF is titrated with a strong base (like NaOH), it will eventually reach an equivalence point where exactly all of the HF has been reacted with exactly the needed amount of NaOH. What will the pH be when HF reaches equivalence point?
(Hint: think about what products will be present and whether they are weak acids, weak bases or neutral...)
pH will be 7.0
pH will be greater than 7.0
pH will be less than 7.0
Homework Answers
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HF is a weak acid (a monoprotic one). When HF is titrated with a
strong base...
Question 35 When titrating a weak monoprotic acid with NaOH at 25°C, the A) titration will...
Question 35 When titrating a weak monoprotic acid with NaOH at 25°C, the A) titration will require more moles of acid than base to reach the equivalence point. B) pH will be less than 7 at the equivalence point. C) pH will be greater than 7 at the equivalence point. D) titration will require more moles of base than acid to reach the equivalence point. E) pH will be equal to 7 at the equivalence point. Question 36
help plwase 2. For a weak acid (e.g., CH.COOH) that is titrated with a strong base,...
help plwase
2. For a weak acid (e.g., CH.COOH) that is titrated with a strong base, (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the equivalence point? 3. For a weak acid (e.g. CH3COOH) that is titrated with a strong base (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the half-equivalence point?
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl...
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
When a weak acid is titrated with a strong base, if the pH at the half-equivalence...
When a weak acid is titrated with a strong base, if the pH at the half-equivalence point is 6.04, what is the Ka of the acid?
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M...
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M NaOH. If a 100.-mL sample of the acid solution required exactly 10. mL of the NaOH solution to reach the equivalence point, what was the original concentration of the weak acid? 2) During the titration on problem (2B), after 5.0 mL of NaOH addition, the pH = 3.68. What is the Ka of the weak acid? please show steps i have an exam tomorrow
A weak acid is titrated with a strong base and the pH vs. volume plot is...
A weak acid is titrated with a strong base and the pH vs. volume plot is shown. Approximately what is denoted with B)? A) The equilibrium of the acid B) The starting pH C) The equivalence point D) The end point E) The pKa of the weak acid D) pH B) A) Volume titrant added O E OB OA Ос OD о Bi E A weak acid is titrated with a strong base and the pH vs. volume plot is...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the...
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the primary standard KHP (potassium hydrogen phthalate, KHC8H4O4) had a potassium iodide impurity of approximately one percent by mass. How would this have influenced the calculated molarity of your sodium hydroxide solution? Would your calculated value be too low, too high, or unchanged? Explain your answer. b. Sketch a typical titration curve for a monoprotic weak acid titrated with a strong base. Label the axes...
An unknown acid is titrated with a strong base (NaOH) to produce the above titration curve....
An unknown acid is titrated with a strong base (NaOH) to produce
the above titration curve. Key points on this graph reveal
important information about the substance and the solution created
with it.
What volume of NaOH is needed to reach the equivalence point
(the point where you added equal moles of NaOH to the
acid)? Select one of the following : ["10 mL", "5
mL", "20 mL", "30 mL", "40 mL", "25 mL", "15 mL", "35 mL"]
...
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write...
1) When a weak acid is neutralized by a strong base, is the neutralization complete? Write the neutralization reaction for HF and KOH. What is the value of Kn (equilibrium constant for neutralization)? (Ka(HF)=3.5*10^-4). If stoichiometric amounts of acid and base are reacted will the resulting solution be acidic, basic, or neutral? Answer: Kn= 3.5*10^10; neutralization reaction is 100% complete since Kn is so large; pH > 7 at equivalence. Just need this explained please :)
Question 35 When titrating a weak monoprotic acid with NaOH at 25°C, the A) titration will require more moles of acid than base to reach the equivalence point. B) pH will be less than 7 at the equivalence point. C) pH will be greater than 7 at the equivalence point. D) titration will require more moles of base than acid to reach the equivalence point. E) pH will be equal to 7 at the equivalence point. Question 36
help plwase
2. For a weak acid (e.g., CH.COOH) that is titrated with a strong base, (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the equivalence point? 3. For a weak acid (e.g. CH3COOH) that is titrated with a strong base (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the half-equivalence point?
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
A weak acid is titrated with a strong base and the pH vs. volume plot is shown. Approximately what is denoted with B)? A) The equilibrium of the acid B) The starting pH C) The equivalence point D) The end point E) The pKa of the weak acid D) pH B) A) Volume titrant added O E OB OA Ос OD о Bi E A weak acid is titrated with a strong base and the pH vs. volume plot is...
An unknown acid is titrated with a strong base (NaOH) to produce
the above titration curve. Key points on this graph reveal
important information about the substance and the solution created
with it.
What volume of NaOH is needed to reach the equivalence point
(the point where you added equal moles of NaOH to the
acid)? Select one of the following : ["10 mL", "5
mL", "20 mL", "30 mL", "40 mL", "25 mL", "15 mL", "35 mL"]
...
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