Answered: Consider the titration of 25ml of…

Consider the titration of 25ml of 0.0823M KI with 0.051M AgNO3, KspAgl =8.3x10-16 Calculate pAg* after adding 39.0 ml 103 Ag* + 103 ====AglO3 O a. 8.2 O b. 6.2 O c. 13.1 d. 12.1

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: 7. A 50.00-ml aliquot of 0.1200 M ethylamine (CH3CH₂NH₂) (Kb = 5.6 x 10-4) is titrated with 0.1000 M…

A: Ethylamine is a weak base and HCl is a strong acid. CH3CH2NH2 + HCl → CH3CH2NH3+Cl- Volume of…

Q: 48. A solution is 1.0x10-20M CO32-, F-, and PO43- each, and 1.0x10-10M Ca2+(Ksp for the calcium…

A: Рreсiрitаtiоn reасtiоns оссur when саtiоns аnd аniоns in аqueоus sоlutiоn соmbine tо…

Q: . In a titration of a strong base with a weak acid at 25oC, the theoretical pH at equivalence point…

A: In a titration of a strong base with a weak acid at 25 oC, the theoretical pH at equivalence point…

Q: Consider the titration of 50.0 mL of 0.0500 M NaCl with 0.100 M AgNO3. Calculate pCl at various…

A: In a titration of NaCl with AgNO3 Silver chloride is precipitated and is known as…

Q: 3.) What is the pH at the equivalence point for the titration of 50.0 mL 0.20 M nitrous acid by 0.20…

Q: Calculate the pl after 50 mL of 0.1 M Nal is titrated with 15.0 mL 0.2 M AGNO, solution? Given (AgI…

Q: Using EXCEL, or other suitable program, prepare plots of pPb?* vs mL titrant added for the following…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Volume of N2OH pH added (ml) 1.00 1.22 1.48 1.85 2.18 2.89 3. 20 3.50 3.90 10 20 30 35 39 39.50…

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

Q: QI/ One of the student wanted to calculate the exact of HCl concentration. He made standardization…

A: The question is based on the concept of acid base titrations. we need to calculate concentration of…

Q: The solubility of Ni(OH)2 in a pH =7.64 solution is_, Ksp Ni(OH)2 =1.6 x 10-16. %3D

Q: Consider the titration of 50.0 mL of 0.0500 M NaCl with 0.100 M AgNO3. Calculate pCl at various…

A: 1,2

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after…

A: Given : Volume of NH2NH2 = 40 ml = 40 / 1000 L concentration of NH2NH2 = 0.200 M concentration of…

Q: he Ka of Benzoic acid (C6H5COOH) is 6.3 x 10-5. A 0.72 M C6H5COOH of 40.0 mL is titrated with 0.48 M…

A: Answer - The correct option is (c) The answer for (1) is 30.0 ml. The answer for (2) is 60.0 ml.…

Q: None

A: To determine the pH at the equivalence point for the titration of trimethylamine ((CH_3)_3N) with…

Q: Consider Titrating a 40 ml of 0.1 M A^3- (Given Kb1= 1x10-4 , Kb2=1x10-9, Kb3=1x10-12) with 0.35 M…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: 25 ml of 0.05M Hg2(NO3)2 was titrated with 0.06M KIO3 Hg2+2 + 2IO3- == Hg(IO3)2 Ksp= 1.3x10-18…

A: Given : Concentration of Hg2(NO3)2 = 0.05 M Volume of Hg2(NO3)2 solution taken = 25 mL = 0.025 L…

Q: Question 23 Which of the following statements is/are true about the equivalence point of a strong…

A: At equivalence point no of moles of acid and base are equal. So, all the strong acid will get…

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 the titration of 25 mL of 0.08230 M KI with 0.05110 M AgNO3. Calculate pAg+ at the…

A: Given in the question,the volume of the KI = 25.00 mlthe molar concentration of the KI = 0.08230…

Q: 8.37 pH 5.0 mL 10.0 mL one: Tartaric acid (H₂C4H₂O6) Maleic acid (H₂CH₂O) Malonic acid (H,C.H, O)…

Q: Part 9: Balance the equation Substitute into the formula with units. Show your answer with units Use…

Q: What ratio of NaF : HF must be added to prepare a buffer with a pH 2.69 Ka = 4.6 x 10-4 pH = pKa +…

A: Given that, pH of NaF: HF buffer solution = 2.69 Ka value of HF = 4.6 x 10-4 Since, pKa = - logKa…

Q: 2. The curve for the titration of 25.0 mL 12 of 0.100 M CSH5N(aq), pyridine, with 0.100 M HCI(aq) is…

A: We have to use date of graph for calculate pKb.

Q: how the following on the graph

Q: Hd saibay 3. A new monoprotic weak acid is synthesized. This acid is titrated with NaOH (V(NaOH…

A: Titration curve: The curve obtained from the plot of pH vs the amount of titrant added. Typically,…

Q: In the the titration of 25.00 mL of 0.1000 M AgNO, with 0.2000 M KSCN; Pcs after the addinon of 12.5…

A: The titration equation is AgNO3 (aq) + KSCN (aq) → AgSCN(s) + KNO3 (aq) Thus AgNO3 and KSCN reacts…

Q: A 40.00-ml aliquot of 0.2000 M HCI is titrated with 02000 M NaOH Calculate the pH of the solution…

Q: 2. Shown in the graph below is the 14- 13 titration curve that results when 12 11 25.0mL 0.200M HCIO…

A: b) if is not a buffer beacuse a stong acid never form a buffer .

Q: Calculate the pH during the titration of 50.00 mL of 0.0500 M NaOH with 0.100 M HCl at 25oC after…

Q: Calculate the pI after 50 mL. of 0.1 M Nal is titrated with 10.0 ml. 0.2 M AGNO3 solution? Given…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

Q: Henry titrated 50.00 mL of 0.25 M nitrous acid with 0.50 M NaOH. What is the pH of the solution at…

A: Given -> Volume of nitrous acid (HNO2)= 50.00 ml Molarity of HNO2 = 0.25 M Molarity of NaOH =…

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: 4. Water with a pH of 9.5 is known to have a buffer of 120mg/L as CaCO3eq. a. Find the molar…

A: TThe objective is to determine the new pH after the addition of the acid and find the maximum volume…

Q: Referring to the figure below, what volume of the titrant was used to reach half-neutralization…

A: The titration curve given is,

Q: The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is

A: Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: 0.0500M

A: The objective of this question is to show the equivalence point is reached when the amount of AgNO3…

Q: In the titration of a strong acid with a strong base, the pH of mixture after equivalence point is…

A: The correct alternative is option C [OH-] = ( NbVb - NaVa )/( Va + Vb ) & pH = 14 - pOH

Q: A 10.0 mL aliquot of 0.100 mol/L NaOH solution was titrated with 0.200 mol/L HCl. what is the pH…

Q: Calculate the molar concentration H3PO4 in a 25.00 ml cola drink, if the concentration of N2OH was…

A: The question is based on the concept of titrations. we have to calculate molarity of phosphoric acid…

Q: Plz do Asap . !

A: Solution-(a) (

Q: The gure below shows a utration table for the tree ammo acid glycine (which is diprotic). At which…

A: Ans is II. At low pH, glycine is in fully protonated form. Here, Carboxyl group (–COOH) has pKa of…

Q: Calculate the pl after 50 mL of 0.1 M Nal is titrated with 20.0 mlL0.2 MAgNO, solution Caen E has…

A: The question is based on the concept of equilibrium. we have to calculate P value for iodide ion 8n…

Q: find the amovnt of buffers and water needed to made 100 mL of 3x buffer of this buffer 1 x bUTfer…

A: Concentration of stock = M1 Volume of stock solution needed = V1 Concentration of diluted 3X buffer…

Q: Calculate the pI after 50 mL of 0.1 M Nal is titrated with 20.0 mL 0.2 M AGNO, solution? Given (AgI…

A: Sodium iodide reacts with silver nitrate to give sodium nitrate and silver iodide. Sodium iodide…

Q: The following results of alkalinity determination for 100 ml sample titrated with 0.02N H,SO.…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

. Consider the titration of 25ml of 0.0823M KI with 0.051M AgNO3, KspAgl =8.3x10-16
Calculate pAg* after adding 39.0 ml I03
Ag* + 103 ====AglO3
O a. 8.2
O b. 6.2
O c. 13.1
O d. 12.1

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

Step 2

Step 3

Step 4

Step 5

Step 6

Step by step

Solved in 6 steps

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 25.00 mL solution of 0.08960 M NaI is titrated with 0.05040 M AgNO3. Calculate pAg+ following the addition of the given volumes of AgNO3. The ?sp of AgI is 8.3×10−17 .35.20 mLpAg+= ?epAg+= 46.40 mLpAg+=
A solution containing 50.0 mL of 10 - 2 M Ca? + ions in the NH4 +/ NH3 buffer whose pH is made to 9 with NH3 is titrated with 0.1 M Na2H2Y solution. Titration a. 5.00; Calculate the [Ca? +] values at 5.50 mL add points. KMY'= KMY.a4 / Fx = 1023
Find the molar concentration
what volume of .65 M strong titrant would be needed to drop pH of a buffer by 0.33 if the buffer was made from 0.0448 moles of pyruvic acid pka 2.55 and 0.0672 moles of the conjugate base pyruvate anion? calculate the pH of the buffer before seeing how much is changing
Suppose titration of 100.00 mL mixture of 0.0500 M in Br + 0.08 M CI with 0.4000 M AgNO3. What is pAg at the second end point? Lütfen birini seçin: a. 9.62 b. 11.43 C. 12.41 d. 4.87 e. 0000 8 8.13
A buffer made up of equal volumes (283.7 mL) of each of 0.688 M A H and 0.715 M A minus. What is p H of the buffer after addition of 13.29 mL of 0.149 M HCI? Ka of HA is 5.090E-5. To avoid rounding errors report your answer with two decimal places. On an exam be sure your scrap work has the correct number of significant figures.
I need the answer as soon as possible
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
You need to use the chart to solve A and B. If you can't solve both could you answer part B? Thank you
A 33.8 mL sample of a 0.400 M solution of NaCN is titrated by 0.160 M HCI. K for CN is 2.0 x 10-6. Calculate the pH of the solution: a. prior to the start of the titration pH = %3D b. after the addition of 50.7 mL of 0.160 M HCl pH = %3D C. at the equivalence point pH %3D d. after the addition of 122 mL of 0.160 M HCl pH = Submit Answer Retry Entire Group 9 more group attempts remaining
Fn 50 PM Wed Apr 19 Alt TA UD ... Alt OH 2. Calculate [HT Jeq if 16.6 mL of 0.120 M NaOH was required to titrate 25.0 mL of the KHT in pure water. Finally, calculate the Ksp. + 96%
A potentiometric titration of acetic acid and 0.100 M NaOH produced the 2nd derivative curve below. Identify the volume of NaOH used to neutralize the acetic acid.