In which of the following titrations would the solution be neutral at the equivalence point? [Hint: For a neutral equivalence point, we need both a strong acid and a strong base as analyte and titrant, respectively.]
HOCl titrated with Ba(OH)2
CH3COOH titrated with NaOH
HClO4 titrated with KOH
Sr(OH)2 titrated with H3PO4
NH3 titrated with HCl
Following is the - complete Answer -&- Explanation: for the given: Question, in.....typed format....
Answer:
Option - ( c ): HClO4 titrated with KOH.
Explanation:
Followingis the complete Explanation, for the above Answer...
We know for a solution to be neutral - at its equivalence point, we require, both the anylate, and the titrant to be strong acid, and strong base, respecively... Now, we will have to check, if any of the given options, satisfy the above mentioned criteria, and therefore will give us our answer...
Following is what we can find about the given options, we have in the question, in the form of a table:
Options ID | Anylate ( acid / base ) | Type of Anylate | Titrant ( acid / base ) | Type of Titrant |
Option - ( a ) | HOCl ( hypochlorous acid ) | weak acid | Ba(OH)2 ( barium hydroxide ) | strong base |
Option - (b) | CH3COOH ( acetic acid ) | weak acid | NaOH ( sodium hydroxide ) | strong base |
Option - (c) | HClO4 ( perchloric acid ) | strong acid | KOH ( potassium hydroxide ) | strong base |
Option - ( d ) | Sr(OH)2 ( strontium hydroxide ) | strong base | H3PO4 ( phosphoric acid ) | weak acid |
Option - (e) | NH3 ( ammonia ) | weak base | HCl ( hydrochloric acid ) | strong acid |
Therefore, as we can see above, the given: Option - (c), as shown in deep brown color is the only option, which satisfies the condition, mentioned in Step - ( 1 ). Therefore, we can certainly say that our answer, would be nothing other than Option - (c), which would satisfy the desired conditions.
---------------------------------------------------------------------------------------------------------------
In which of the following titrations would the solution be neutral at the equivalence point? [Hint:...
In which of the following titrations would the solution be neutral at the equivalence point? Select one: a. NH3 titrated with HCl b. Sr(OH)2 titrated with H3PO4 c. HOCl titrated with Ba(OH)2 d. CH3COOH titrated with NaOH e. HClO4 titrated with KOH
E. Titration calculations 1. A 25.0-ml sample of 0.100 M HCl is titrated with 0.125 M NaOH. How many milliliters of the titrant will be need to reach the equivalence point? 2. A 25.0-ml sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCI. How many milliliters of the titrant will be need to reach the equivalence point? 3. For the following titrations, determine if the equivalence points will be acidic, basic, or neutral i. NH3 titrated with HCI...
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.) (a) 101.5 mL of 0.19 M HCO2H (Ka= 1.8 ✕ 10-4) titrated with 0.19 M KOH (b) 104.1 mL of 0.18 M (C2H5)3N (Kb = 4.0 ✕ 10-4) titrated with 0.36 M HClO4 (c) 100.9 mL of 0.47 M HClO4 titrated with 0.24 M NaOH
For the following titration, determine whether the solution at the equivalence point is acidic, basic or neutral and why: KOH is titrated with HI(aq) basic because of hydrolysis of K+ basic because of hydrolysis of KOH acidic because of hydrolysis of OH- acidic because of hydrolysis of HI neutral salt of strong acid and strong base
Which one of the following titrations will have an equivalence point with a pH of 7? options: HNO3 with KOH NaC2H3O2 with RbOH HF with NaOH none of these HCl with NH3
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....
Learning Goal: To learn about titration types and how to calculate pH at different points of titration. In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration...
Predict where the pH will lie at the equivalence point for the following titrations a. Strong Acid titrated with Strong Base b. Strong Acid titrated with weak base c. Weak Base titrated with Strong Acid d. Weak Acid Titrated with Strong Base e. Strong Base titrated with weak acid
3. Predict qualitatively what the pH will be at the equivalence point of the following three titrations at 25 °C (pH >7, or pH = 7, or pH <7). Briefly explain your reasoning. i. HBrO titrated with NaOH: ii. C2H5NH2 titrated with HNOZ: iii. KOH titrated with HCIO:: iv. HNO2 titrated with Ba(OH)2: v. NH3 titrated with HCIO:
Predict whether each solution will be neutral, basic, or acidic at the equivalence point of each titration. a. An aqueous solution of NaOH is titrated with 0.100 M HCl. b. An aqueous solution of ethylamine (CH3CH2NH2) is titrated with 0.150 M HNO3 c. An aqueous solution of aniline hydrochloride (C6H5NH3+Cl−) is titrated with 0.050 M KOH.