A triprotic acid is titrated with KOH. What species are NOT in solution to any large extent between the 1st and 2nd equivalence points? Select all that apply. O H3A O HA2- A3-
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Q: 2) The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…
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Q: Please explain step by step and legible writing Thanku!
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A: We will see the maximum buffering capacity for a weak acid. You can see details solution below.
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A: Note: As per company policy we are supposed to attempt first question only. Please repost other…
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A: This is a case of acidic buffer solution. Moles of HCOOH = (185*0.1)/1000 = 0.0185 Moles of HCOONa…
Q: You are titrating 20.00 mL of 0.1000 M acetic acid with 0.1000 M NaOH. Instead of using an…
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Q: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…
A: Acetic acid dissociates gives H+ ion and acetate ions.
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Q: A 10.0-mL solution of 0.300 M NH3 is titrated with a 0.100 M HCI solution. Calculate the pH af- ter…
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Q: Answer the following 14 question relating to the 12 titration curve you have just plotted using the…
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Q: The following plot shows a titration curve for the titration of 1.00L of 1.00M diprotic acid H2A
A: Since H2A is a diprotic acid and it can gave two H+ ions in the solution therefore it has two…
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Q: Sketch a titration curve of a triprotic weak acid (Ka’s are 5.5x10-3, 1.7x10-7, and 5.1x10-12) with…
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Q: after titrating
A: Mmol of Acid = 0.10 × 40 = 4.0 mmol Mmol of KOH = 20 ×0.20 = 4.0 mmol It forms Amphoteric salt,…
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Q: Equivalence Point pH = 7
A: equivalence point is the point at which the concentration of analyte and the titrant is equal. at…
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Q: Titrate 50 ml of a 0.150 M solution of HBr with 0.00 ml of 0.150 M KOH.What is the pH initially?
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Q: In weak acid-weak base titration, the equivalence point is a. above pH 7 b. at pH 7 c. bellow pH 7…
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Q: 1. What is the pH aft er adding 18 ml of 0.12N sodium hydroxide? 2.What is the pH at equivalence…
A: Solution: 4. Moles of NaOH used for 18 mL = molarity x volume/1000 = 0.12 x 18/1000 = 0.00216 moles…
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- Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
- A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________MWhat is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
- When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. ÂConsider 1000. mL of a 1.00 104-M solution of a certain acid HA that has a Ka value equal to 1.00 104. How much water was added or removed (by evaporation) so that a solution remains in which 25.0% of HA is dissociated at equilibrium? Assume that HA is nonvolatile.
- A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein end point. Is the acid monoprotic, diprotic, or triprotic?A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.