Given 20.00 ml of 0.1000M HCN (Ka=4.9 x 10-1⁰ ) titrated with 0.0500 M NaOH.Calculatea.b.C.d.VNaOH at equivalence pointpH at equivalence pointpH when the V₁₁titrantpH when additional10.00 ml of titrant is added past the equivalence pointis ½ that in letter a

As per our company guidelines we can answer only three subparts. Kindly repost the question…

Answered: Given 20.00 ml of 0.1000M HCN (Ka=4.9 x…

Given 20.00 ml of 0.1000M HCN (Ka=4.9 x 10-10) titrated with 0.0500 M NaOH. Calculate a. b. C. VNaOH at equivalence point pH at equivalence point pH when the Vtitrant is ½ that in letter a

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Use the References to access important values if needed for this question. How many grams of solid…

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

A: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its…

Q: A 25.0mL sample of 0.125M pyridine is titrated with 0.100M hydrochloric acid. Calculate the pH at…

A: From given datas With Kb of pyridine, at different volume of added acid pH is calculated…

Q: Given: The pH of the buffer is 4.88 made by combining 0.500 L of 0.380 M HC3H5O2 (Ka=1.30X10-5) and…

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: 10- 8- 6- OH 2- H30¹ **** 10 strong acid strong base B A ... 20 30 40 Volume titrant (mL) Aside from…

A: Answer:Since, on adding the volume of titrant, pH of the solution is decreasing, therefore it is…

Q: 25.0 mL of 0.100 M weak acid solution is titrated with 0.200 M NaOH. The Ka of the acid is 1.4 x 10…

A: First, the volume of NaOH required to reach the equivalence point in titration is determined. The…

Q: A scientist wants to prepare 500 ml of 500 mM formate buffer pH 3.00. The pKa for formic acid,…

Q: D)

A: Since,you have posted a question with multiple sub-parts,we will solve the first three sub-parts for…

Q: Formic acid, HFor, has a Ka value of 1.8 # 10-4 . You need to prepare 150 mL of a buffer hav-ing a…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: A 25.0mL samnple of a solution of an unknown compound is titrated witha 0.115M NaOH solution. The…

A: For the both at Equivalence point and at Pka its pH is same Around = 8.5

Q: Which of the following would be best for a buffer with a pH of 7.5? a. HF/F- b. H3PO4/H2PO4- c.…

A: The pH of the buffer given is 7.5.

Q: Question 5 of 7 What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of…

A: Given -> Volume of HF = 200.0 ml = 0.209 L (1L = 1000ml) Molarity of HF = 0.200 M pH = 4.30 Ka…

Q: ketch a titration curve for the titration of a weak base with a strong acid. Label the axes and cate…

A: The question is based on the concept of titrations. we are titrating a weak base with a strong…

Q: 14 12 10 pH 6. 10.0 20,0 30,0 40.0 50.0 60.0 70.0 Volunic added (nmL) The figure shows the titration…

A: Interpretation - To tell about that which is the strongest base as the figure shows the titration…

Q: Consider this acid hase titration curve OH H₂O' 14 2 12 104 P 0 strong acid *** weak acid A 10 B…

A: Answer:Since, on adding the volume of titrant, pH of the solution is increasing, therefore it is…

Q: Calculate pH at 0 mL NaOH added, 6.5 mL NaOH added, 14.25 mL added, and 23.50 mL added. 120 mL of…

A: we need to calculate the pH of solution

Q: Calculate the ApH of 20.00 mL of a buffer containing 0.36 M HC2H3O2 and 0.46 M C2H3O2 when 5.00 mL…

Q: What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.609 mol of NaA in…

A: Buffer solution :- A solution which resists the change in its pH value by the addition of small…

Q: 1. This titration curve could represent 20 ml of 0.1 M with 0.1 M NaOH. The buffer region(s) is/are…

A: We are given the titration curve for the titration of an acid with strong base, NaOH.

Q: GIVEN: 0.35 M HAC 0.25 M Na acetate Pka = 4.76 Buffer solu. volume= 300ml 1. Calculate pH of buffer…

A: Given,Molarity of acetic acid ( HAc ) ( CH3COOH ) = 0.35 MMolarity of Na acetate ( CH3COONa ) =…

Q: 30.0 mL of 0.200M H2SO3, a diprotic acid is titrated with 0.100M NaOH. a) Calculate the volume…

A: The reaction taking place between H2SO3 and NaOH is- H2SO3 + NaOH→NaHSO3 + H2ONaHSO3 + NaOH→Na2SO3 +…

Q: A given indicator has Ka, Ind=7.9x10-9. This indicator would best be used for... a titration…

Q: e pH a

Q: 0.0 mL of 0.600 M KOH is titrated using 0.400 M H2SO4. What is volume of H2SO4 needed to reach the…

A: Answer is 30.0 ml

Q: B)

A: The milliliters of NaOH are needed to reach the equivalence point is to be calculated. The…

Q: Consider that titration of 30.0 ml of 0.265m weak base B (Kb = 1.3×10^-10) with 0.150M HI. a) What…

A: Given: Volume of the weak base = 30.0 mL Concentration of the base = 0.265 M Concentration of HI =…

Q: 10. Which of the following mixture(s) is a buffer: a. 25mL 0.1M NaOH mixed with 25mL 0.1M NaOAC. c.…

A: Here we have to predict buffer solution from the following given mixture. To be a buffer solution…

Q: When titrating a strong monoprotic acid and KOH at 25C, the a. pH will be less than 7 at the…

Q: d. A solution containing 1.00 mol of N2H4 (Kb = 8.9 x10-7) and 0.005 mol of HCl in 1 L of water is a…

Q: Which of the following will cause the largest change in pH of a 50.0 mL, 0.1 M HN3/N3 buffer pH 5.0?…

A: pH of the buffer solution can be found out using H-H equation.

Q: The pH at the equivalence point is estimated as 7.93. Which indicator is most suitable for the…

A: The reaction between HF and NaOH is HF (aq) + NaOH (aq) -----> NaF (aq) + H2O (l) Given that pH…

Q: How many mL of 0.2 M sodium acetate and 0.2 M acetic acid are needed to prepare 1 liter of 0.1 M…

A: Here we are required to find the volume of sodium acetate and acetic acid needed to prepare 1L of…

Q: 5. Use the titration curve to the right to answer the following questions A. What is the pH at the…

Q: What mass of sodium benzoate should you add to 154.0 mL of a 0.13 mol L benzoic acid solution to…

Q: A 13.0 ml solution of weak base with Kb = 1.33×10-3 (at 25°C) with concentration of 0.086 mol L1 was…

Q: Calculate the pH when 2.0 M HCl is used to titrate 50 mL of 1.0 M NH3 (Kb = 1.8 x 10-5 ). a.) before…

A: This is problem of titration of weak base and strong base which goes through formation of basic…

Q: A 25.0mL sample of 0.125M pyridine is titrated with 0.100M hydrochloric acid. Calculate the pH at…

Q: C)

Q: How many moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a buffer…

A: We have, The number of moles is calculated by using the following expression. So, No. of moles =…

Q: 11. A 35.0 mL sample of 0.100 M acetic acid is titrated with a 0.150 M NaOH solution. The Ka of…

A: pH is an indicator to check the hydrogen ion’s amount concentration is available in a solution. The…

Q: Chem 129 Topic Set 7 Variations of titration and Buffers G. How would you make 350mL of a buffer…

A: Desired pH of the buffer = 9.00 Desired volume of the buffer = 350 mL Desired concentration of the…

Q: In the titration curve below, which species would NOT be in solution at Point B? Unknown Solution…

A: In the given graph, at B point pH=11

Q: 5. Use the titration curve to the right to answer the following questions A. What is the pH at the…

Q: Over much of the titration curve, the pH lies within 1 pH unit of the pk- In this range, the change…

A: Given:Part A:Concentration of NH4Cl = Part B:For NH4Cl:For NaOH:Part C:For NH4Cl:For NOH:The pH of a…

Q: You are titrating 20.00 ml of 0.200 M HOAc with 0.200 M NaOH. What is the pH at the equivalence…

Q: The ionization of the first proton from H₂ SeO4 is complete ( H₂ SeO4 is a strong acid); the…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: 100 mL of a buffer that consists of 0.20 M NH3 and 0.20 M NH4Cl is titrated with 25 mL of 0.20 M…

A: Given,Volume of buffer solution = 100 mLMolarity of NH3 = 0.20 MMolarity of NH4Cl = 0.20 MMolarity…

Q: How many grams of solid potassiumfluoride should be added to 2.00 L of a 0.236 M hydrofluoric acid…

Q: To prepare 1 liter of 0.10 M acetate buffer at PH 5.20.I need to mix _____g of CH3COONa molecular…

A: Any particular amount of acidic species or basic species which is added to any buffer solution…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Given 20.00 ml of 0.1000M HCN (Ka=4.9 x 10-1⁰ ) titrated with 0.0500 M NaOH.
Calculate
a.
b.
C.
d.
VNaOH at equivalence point
pH at equivalence point
pH when the V₁₁
titrant
pH when additional10.00 ml of titrant is added past the equivalence point
is ½ that in letter a

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 300 ml 1.6 M solution of an acid (HA), has a pH of 2.4 at 25oC. From the given information, could you: a. Find the full equivalency pH? b. Find the Ka of the acid? c. Treat this like a buffer? Explain:
Consider the titration of a 25.0mL sample of 0.195M acetic acid (CH3COOH) with 0.300M NaOH. How many mL of NaOH is required to reach the equivalence point? The Ka of acetic acid is 1.8x10-5.
A 50.0 mL of 0.120 M HCN (Ka HCN = 6.20 x 10-10) is titrated with 0.100 M NaOH. The pH at equivalence point is a.) 0.2 b.) 10.8 c.) 7.0 d.) 3.2
30.0 mL of 0.400 M KOH is titrated using 0.300 M H2SO4. What is volume of H2SO4 needed to reach the equivalence point? 30.0 mL 40.0 mL 20.0 mL 15.0 mL
In a potentiometric titration of 80ug of monoprotic acid requires 15.00uL of 0.100N NaOH to reach the equivalence point. What is the acids equivalent weight?
2. Calculate the volume of the salt to be used in the preparation of 200 ml of the following buffer solutions. Show computations below. BUFFER DESIRED NUMBER pH 456N 7 8 2.10 SITO 4.40 6.90 7.18 9.45 8.25 0.1M SOLUTIONS QWOL CH3COOH/CH3COONa NaH₂PO4/Na₂HPO4 NaH₂PO4/Na₂HPO4 NH4CI/NH3 NH4CI/NH3 pka 4.70 6.80 6.80 9.30 9.30 VOLUME OF SALT (ml)
4. You are titrating 50.0 ml of 0.100 M Na:CO, with 0.400 M AGNOS. Calculate the pAg* values.. a) 1.0 ml. before the equivalence point b) at the equivalence point c) 1.0 mL after the equivalence point
A 24.0 mL sample of 0.115 M sulfurous acid (H,S03) is titrated with 0.1019 M KOH At what added volume of base solution does the first equivalence point occur? Express your answer in mililiters to three significant figures. V. mL Submit Request Answer Vorue nertlel
Calculate the pH during the titration of 20.00 mL of0.1 M NaOH with 0.100 M HCl after theaddition of the following volumes of reagent:a. 0.00 mLb. 10.00 mLc. 15.00 mLd. 20.00 mLe. 24.5 mLf. 25.00 mLg. 30 mLh. 35 mL
Be sure to answer all parts. Find the pH of the equivalence points when 28.9 mL of 0.0850 M H₂SO3 is titrated with 0.0312 M NaOH. pHlst PH²nd
16. Calculate the pH at the equivalence point in the titration of 25 mL of 0.10 M formic acid with a 0.1 M NaOH solution (given that pka of formic acid = 3.74). A. 4.74 B. 8.74 C. 8.37 D. 6.06 17. When a 0.20 M solution of acetic acid is neutralized with 0.20 M NaOH in 0.50 L of water, the pH of the. resulting solution will be (given that pKa for CH3COOH = 4.74) A. 12.67 B. 7.87 C. 8.87 D. 7.00 18. Calculate the equivalent weight of Na2CO3 when it is titrated against HCI in the presence of phenolphthalein. A. 106 B. 53 C. 26.5 D. 212
A 20.0 mL sample of 0.115M H2SO3 is titrated with 0.1014 M KOH. At what volume (of added base) does each equivalence point occur? a. 25.0mL for the first equivalence point and 50.0mL for the second equivalence point. b. 33.2mL for the first equivalence point and 66.4mL for the second equivalence point. c. 22.7mL for the first equivalence point and 45.4mL for the second equivalence point. d. 20.0mL for the first equivalence point and 40.0mL for the second equivalence point.