Answered: You have a 1.25 L solution with 2.14 g…

Science

Chemistry

You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the Kb of NaIO?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 76QAP: A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a...

See similar textbooks

Related questions

Q: What mass of Ca(OH)2 is required to neutralize 50.00mL of 0.180 M HCI?

A: Balanced chemical equation for the reaction between hydrochloric acid and calcium hydroxide is,

Q: A solution is made by dissolving 35.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Ba(NO2)2 is a salt which is mixture or strong base or weak acid so use pH of salt formula to get…

Q: What is the pH and pOH of a solution with a volume of 5.4 L that contains 15 grams of hydrochloric…

A: To calculate the pH and pOH , firstly molarity should be calculated to see how many moles are…

Q: What is the pH of a 0.0520 M solution of HONH;CI (Kb of HONH2 is 1.1 x 10-8)?

A: HONH3Cl is a salt of weak base HONH2 and strong acid HCl Recall the following expression to…

Q: A solution is made by dissolving 26.5 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 ×…

A: Given that, Weight of Ba(NO₂)₂ = 26.5 g Weight of Ba(NO₂)₂ = 26.5 g/261.337 g/mol = 0.1014 mol…

Q: If 0.235 g of KHP (potassium hydrogen phthalate) require 15.5 mL of NaOH solution to neutralize it,…

Q: A 1.2· 102 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of 1.62 O 4.2- 10-13 12.38 O 12.08 O…

Q: How many mL of 0.40 M NaOH should be added to 10.0 g of tris hydrochloride (pKa 8.072) to give a pH…

A: Given data,Molarity of NaOH=0.40MMass of tris hydrochloride=10.0gMolar mass of tris…

Q: What is the pH of a 0.320 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

Q: If it takes 25.22 mL of H3PO4 to neutralize 35.22 mL of 0.313 M Ba(OH)2, what is the molarity of…

A: Given, Molarity of Ba(OH)2 = 0.313 M Volume of Ba(OH)2 = 35.22 mL Volume of H3PO4 = 25.22 mL…

Q: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca1OH22?

A: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca(OH)2?

Q: what volume of 0.134m/L of calcium hydroxide is needed to completely neutralize 72.3ml of 0.475mol/L…

Q: A 1.0 M solution of HNO3 was used to neutralize 100.0 ml of 0.20 M Ba(OH)2. Volume of HNO3 is 20ml.…

A: Titration of strong acid versus strong base- In solution the number of mole of [H+] from acid…

Q: What is the concentration of ion or molecule in the solution of 0.0150 M C6H12O6?

A: Given: 0.0150M C6H12O6The given molar solution contains molecules of C6H12O6 since no ions are…

Q: 6.5 g of sodium acetate was dissolved in 100 mL of water to give a final volume of 106 mL. If the Ka…

A: Sodium acetate dissociates in water into sodium and acetate ions. Sodium ions react very little with…

Q: er the following solutions are acidic, basic, or nearly neutral: (a) NaBr, (b) K2SO3, (c) NH,NO2,…

Q: What is the pH of a 0.830 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The chemical equation may be written as: The given data is: Concentration of Ca(NO2)2 =0.830M Ka of…

Q: Propionic acid, CH3CH2COOH, has a Ka = 1.34 x 105. If 10.00 mL of 0.080 M propionic acid is mixed…

Q: What is the pH of a 0.320 M solution of Ca(NO,), (Ka of HNO, is 4.5 × 104)?

A: For HNO2 , pKa = -logKa = -log (4.5 x 10-4 ) =…

Q: The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (c)…

A: The reaction can be given as follows: HClO(aq)+NaOH(aq)→NaOCl(aq)+H2O(l) Molarity of HClO = 0.015 M…

Q: What is the pH of a mixture of 0.042 M NaH2PO4 and 0.058 M Na2HPO4?

A: Given : Concentration of NaH2PO4 = 0.042 M Concentration of Na2HPO4 = 0.058 M

Q: A weak base is dissolved in water with a concentration of 0.200 mol/L. The Kb value of the base is…

A: Given :- initial concentration of base = 0.200 mol/L Kb of base = 9.75 × 10-4 To…

Q: What is the pH of a solution of 0.075M HNO2 and 0.030 NaNO2?

Q: if magnesium hydroxide were used instead of naoh how many moles would it take to combine with three…

Q: What is the pH of a 0.0760 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: Given salt is a mixture of W.B + SA HONH3Cl it undergo salt hydrolysis It's pH = 7 - 1/2(pkb +…

Q: What are the concentrations of H3O+ and OH− in tomatoes that have a pH of 4.10 ?

Q: 12. The hydrogen ion concentration of a lemon is about 0.01. What is its pH?

A: pH is defined as the negetive logarithm of Hydrogen ion concentration. That is, pH = -log[H+]

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: A 1.2 · 102 M aqueous solution of Ca(OH)2 at 25.0 °C has a pH of, O 12.38 O 12.08 O 1.62 O 2.4 · 102…

Q: What volume of 0.50 M KOH would be required to neutralize completely 500 mL of 0.25 M H 3 PO 4…

A: Given data contains, Molarity of potassium hydroxide is 0.50 M. Volume of H3PO4 is 500 mL. Molarity…

Q: What is the pH of a 0.560 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.560 M And Ka of HNO2 = 4.5 X 10-4 Since Ca(NO2)2 is a…

Q: if 25.00 ml of citric acid solution is titrated with 28.12 ml of 0.1718 N KOH, what is the…

Q: 25. Mik of nmagnesia, Mg(OH),, has a pH of 10.5. Calculate the hydronium jon concentration of the…

A: Given pH for milk of magnesia Mg(OH)2 =10.5 We know, pH=-log[H3O+] 10.5 = -log[H3O+] Taking antilog…

Q: What is the concentration of sodium ions in 0.300 M NażSO,?

A: Given: 0.300M Na2SO4 1 mole of Na2SO4 has 2 moles of Na+ Then,

Q: What volume of 0.3M HNO3 will be required to react and neutralize 24ml of 0.25M KOH?

A: Consider the given information is as follows; Molarity of HNO3=MHNO3 = 0.3 M Volume of HNO3=VHNO3 =…

Q: On dissolving 7.258 gm of HCN (Ka=7.2x10 1) in water, the solution become 100 ml so the degree of…

A: HCN is a Weak acid the degree of dissociation of a weak acid or base or an electrolyte was explained…

Q: 650.0 mL of HBr gas at 21.0 °C and 1025 mm Hg is absorbed completely into a solution that was…

A: Given, Volume = 650 ml, temperature = 21℃, pressure = 1025 mm Hg = 1.35 atm, mass of water(solvent)…

Q: If a 1.5 L sodium hydroxide solution contains 38g of NaOH, what is the pH of the solution?

A: We have to calculate the pH of Solution.

Q: What volume of 2.25-M H2SO4 should be diluted with water to form a 1.25 liters of 1.5 molar of the…

A: The process of dilution is defined as the process in which a solution with a lower concentration is…

Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

Q: A 0.539 M solution of oxalic acid (pK, = 1.23) is prepared. Determine the pH of the !3! solution.…

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: 10. Nitrous acid (HNO2) is a weak acid with a Ka = 4.0 x 104. If 112 mL of a 0.100 M KOH solution…

A: Answer: In this question we have to find out the pH of a buffer solution made of nitrous acid and…

Q: What is the pH of a 0.450 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

Q: What substance(s) have a pH most similar to that of water (pH 7)?

A: Salt of strong acid and strong base have a pH similar to that of water i.e. pH = 7.

Q: What volume of 1.556 mol L solution of LIOH is required to make 5.40 L of a solution with a pH =…

A: Initial Molarity of LiOH ; M1 = 1.556 mol.L-¹ = 1.556 M V1 = volume of 1.556 M of LiOH solution…

Q: How many mols of HBr are used to neutralize 18.66 mL of a 0.2299 M Ca(OH)₂ solution?

Q: 6 A solution of NaOH has a pH of 10.50. How many grams of CaO should be dissolved in sufficient…

A: To solve this problem we have to first calculate the concentration of OH- by using the pH of NaOH…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the K_b of NaIO?

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?
A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution, What is the pH after 26.0 mL of base is added? The K, of benzoic acid is 6.3 · 105, O 11.47 O 2.54 O 7.00 4.18 4.22 O O O O O
(a) A 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH is titrated into the solution until the pH is exactly 5.0. What is the concentration of the titrant (NaOH)? (b) In the second step, enough 5.85 M nitric acid is added to the solution after the titration in part (a) is complete until the pH is one unit lower than the pKa of acetylsalicylic acid. What volume (mL) of nitric acid was added?
What is the number of moles of 10.0 g NH₄Cl? What is the molar concentration of NH₄Cl? What is the pH of the buffer solution?
A 1.00 L solution contains 0.383 M HA (K₂ = 4.52 · 10−4) and 0.790 M NaA. What is the pH of this solution? What is the pH if 0.121 L of 0.178 M KOH is added to the solution be? What is the pH if 0.242 L of 0.178 M KOH is added to the solution be? 3.65
A buffer solution is made that is 0.449 M in H₂S and 0.449 M in NaHS. If Ka1 for H₂S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Use the References to access important values if needed for this question. Write the net ionic equation for the reaction that occurs when 0.093 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + Submit Answer + Retry Entire Group 8 more group attempts remaining
What volume of 0.317M KOH solution will be required to titrate 25.00mL of 0.285M HNO3? What mass of Ca(OH)2 is required to neutralize 5.00mL of 0.180M HCl?
4. How does the pH of each of the following solutions change when 5.0 mL of 1.0 M NaOH (a strong base) is added? Fill in the table. Give your answers with 2 decimals. Initial pH Final pH after adding NaOH Solution (a) 100.0 ml water (b) (c) 100.0 mL 0.150 M HNO2 (a weak acid) (Given: Ka = 4.5 × 10-4) 100.0 mL solution of 0.150 M HNO2 and 0.100 M NaNO₂
A chemistry graduate student is given 250. mL of a 1.40M ammonia (NH3) solution. Ammonia is a weak base with K-1.8x10 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.17? What mass of NH, Br You may assume that the volume of the solution doesn't change when the NH4Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
1. If 30.00 ml of a 0.300 mol/L of a weak acid, CH,CO,H (aq), is titrated with a 0.300 mol/L NaOH(aq), a strong base, determine the amount/moles and pH of the remaining acid after K, = 1.8 x 10* (a) 0.00 mL of NaOH is added (b) 10.00 mL of NaOH has been added. O at equivalency point when 30.00ml of NaOH was added. (d) Explain why the pH differs in (b) and (c)
2) A buffer solution contains 0.339 M ammonia. If 0.0248 moles of hydrochloric acid are added to 125.0 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding hydrochloric acid.) Kb for NH3 = 1.8 X10 M
A chemistry graduate student is given 300. mL of a 0.60 M ammonia (NH,) solution. Ammonia is a weak base with K, = 1.8 x 10. What mass of NH,Br should the student dissolve in the NH, solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. do Ar x10 ?