Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation:10 + H20 = HIO + OHK, for hypolodite ion = 0.00044.Calculate the [H'1 and pH of a 0.971 M solution of Nal0.Now calculate the [H'1 and pH of a 0.017 M solution of Nalo.40

Given Reaction:- IO- + H2O <----------> HIO + OH- Kh = 0.00044 Kh = [HIO ] [ OH- ] / […

Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation: 10 + H20 = HIO + OH K, for hypoladite ion = 0.00044. Calculate the [H'1 ancd pH of a 0.971 M solution of Nalo. Now calculate the (H] and pH of a 0.017 M solution of Nalo.

Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation: 10 + H20 = HIO + OH K, for hypoladite ion = 0.00044. Calculate the [H'1 ancd pH of a 0.971 M solution of Nalo. Now calculate the (H] and pH of a 0.017 M solution of Nalo.

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: What volume of (0.45 M) Ca(OH)2 must be added to 50 mL of 0.25-M (KOH) to give a solution 0.8 M in…

A: Concentration of Ca(OH)2 =0.45M Valume of KOH = 50ml Concentration of KOH =0.25M Concentration of…

Q: 1. Complete and balance the following equations for acid-base reactions: NH3 HNO3 > NaHCOз HCI ->…

A: Interpretation - To complete and balance the following equation for acid -base reactions -…

Q: What is the equilibrium constant of the HSO4-ion, if [H3O+] = 0.027 M; [HSO−4] =0.29 M; and [SO2−4]…

A: The Complete and balanced chemical equation is given as,

Q: Calculate the pH for the following concentration: [H3O+] = 2.19 x 10-5 M.

Q: Determine the voltage of a galvanic cell composed of Pb(s) in a 1.00 M solution of Pb²+, and Ni(s)…

Q: When COCI2 is placed in a container with a pressure of 4.1 atm, determine the equilibrium…

A: Since you have posted multiple questions as per guidelines we can answer only one per session . If…

Q: Complete the table. (All solutions are at 25 °C.) Solution [H3O+] [OH-] pH 1 3.19 2 3 4 3.2 x 10-9…

Q: Done 7 Part A Calculating pH What is the pH of an aqueous solution with the hydronium ion…

Q: A substance has a pH of 5.3. Their [H*] is

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: Calculate the H+] and pH of a 3.05 x 10¬4 M nitrous acid solution. The Ka of nitrous acid is 7.10 x…

Q: . Calculate the pH of a 0.0368 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

A: HNO2 is a weak acid and does not undergo complete dissociation in solution.

Q: Calculate the pH of a 0.022 M RbOH solution.

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: A triprotic acid is an acid that has three dissociable protons. When such an acid undergoes stepwise…

Q: Calculate the pH for 0.0150 M H₂CrO solution. For H₂CrO, Ka₁ is very large and Ka₂ is 3.10 x 10-³.

A: Given , Concentration of H2CrO4 =0.0150 M

Q: 18 of 21 I Review | Constants | Periodic Table The temperature for each solution is carried out at…

A: Given that: Mass of HCl = 0.80g Molar mass of HCl = 36.5g/mol Volume of solution = 3.5L

Q: If you have a solution of 0.10 M sodium acetate (NaOAC) and the Ka-1.8 x 10³ Calculate the pH of…

Q: Calculate the pH at 25 °C of a 0.46M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A: Given data :

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

Q: 12 . What is the expected pH of a 0.015 M solution of boric acid (assuming 100% dissociation) ?

Q: According to the table in the text, hydrogen fluoride (HF) has a pK, of 3.2. If a solution of HF is…

A: According to the Henderson-Hasselbalch equation for a buffer containing a weak acid (e.g., HF) and…

Q: Classify the compounds according to the pH condition that would improve their solubility in water.…

A: Solubility depends upon environment.

Q: The molar concentration of H3O+ was measured at 25 ° C. The pH and pOH should be calculated for the…

Q: What is the pH of a solution that is 0.080 M in NaClO at 25 °C? The Ka for HClO is 4.0*10^-8

Q: Calculate the [H+] and pH of a 1.97 × 10-4 M nitrous acid solution. The K, of nitrous acid is 7.10 x…

A: Given, Concentration of the nitrous acid (HNO2) solution (C) = 1.97 × 10-4 M Ka of nitrous acid…

Q: Calculate the PH and the POH for a .66 moles solution of NH3 Ki for NH3 = 1.9 x 10-5

A: To calculate the pH and pOH of the solution, we need to first determine the concentration of…

Q: Determine the pH of a solution that is 0.00539 M HCl and 0.0516 M HC1O₂. The K, of HCIO, is 1.1 x…

Q: Calculate the pH of a solution that is a mixture of 0.030M HNO3, 0.55M CH3COOH, and 0.015M HI. Ka…

A: Given data : HNO3 = 0.030 M HI = 0.015 M CH3COOH = 0.55 M

Q: Calculate the pH of a 0.299 M NH, solution. NH, has a Kp = 1.8 × 10-5. pH =

A: pH =11.366

Q: 10. Calculate the pH of a 0.250 M solution The Ka of HCIO is 2.9x10-8.

Q: 2. Suppose a 0.0500M solution of HNO, was created Write the dissociation reaction for this compound.…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Calculate the pH of a 0.11 M solution of HCIO, with Ka = 3.5x10-8.

Q: Calculate the pH of a 0.58 M CH3CO2H solution

Q: Calculate the [OH-] and pH given that it is a mixture of 0.12 M in NaNO2 and 0.23 M in Ca(NO2)2

A: Given, A mixture of 0.12 M in NaNO2 and 0.23 M in Ca(NO2)2

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10~7. Calculate the pH of a 4.0…

Q: The Kb for four bases are = 1.6 x 10$, CO;²- = 2.1 × 10-4, NH3 each of these weak bases were…

A: We have to predict the order of pH from high to low.

Q: Hydrazine, N₂H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K, of…

A: moles of Hydrazine = 4.75 × 10-3 molVolume of the solution = 0.500 LKb of Hydrazine = 9.1 × 10-7pH…

Q: Calculate the pH and pOH of aqueous solutions with the following concentration: (in the image)

A: The question is based on the concept of PH and pOH calculations. pH is defined as negative…

Q: The ionization constant of nitrous acid is 4.5 x 10-4. Calculate the pH of 0.04 M solution of…

A: Ka of HNO2 = 4.5*10-4[HNO2] = 0.04 MpH = ?

Q: NH3 is a weak base (K, = 1.8 × 10-') and so the salt NH4CI acts as a weak acid. What is the pH of a…

A: Given, Concentration of NH4Cl solution = 0.075 M Kb for NH3 = 1.8 × 10-5 pH of the solution = ?…

Question

Salts of hypoiodite ion behave as a weak base, undergoing hydrolysis in water according to the equation:
10 + H20 = HIO + OH
K, for hypolodite ion = 0.00044.
Calculate the [H'1 and pH of a 0.971 M solution of Nal0.
Now calculate the [H'1 and pH of a 0.017 M solution of Nalo.
40

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

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 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

8. Calculate the pH of a solution with [H3O']= 9 × 101 M.
calculate the ph of a 2.00M solution of HNO2. The KA for nitrous acid is 4.5 x 10^-4
Calculate the pH of a solution that’s 0.65 M in NaNO2 and 0.40 M in HNO2. (HNO2, Ka = 4.45 × 10–4 ).
I Review | Constants | Periodic Table Learning Goal: Part A To calculate pH and use it as a measure of acidity. The pH expresses the molar concentration of hydronium ions in an aqueous solution on a logarithmic scale: What is the pH of an aqueous solution with [H30+] =2x10-14 M? Express the pH numerically using one decimal place. pH = -log[H3O+] • View Available Hint(s) [H3O+] = 10-pH As pH decreases, acidity increases. As pH increases, acidity decreases. • Acidic solution: pH 7 pH = Submit Part B Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is the molar concentration of H3O+ in a cola that has a pH of 3.120? Express your answer with the appropriate units. • View Available Hint(s) [H3O*] = Value Units Submit
For 0.265 M HClO solution. The Ka of HClO is 2.9 X 10-8. The pH of the solution is 8.766
Calculate the pH of a solution that has a 0.0025 M [H3O] +
23.
Calculate the PH and POH for a .023 mole solution of HBrO2 Ki for HBrO2 = 2.1 X 10-4
Calculate the pH and concentration of species present in a polyprotic acid solution. For a 9.03x10 M solution of H,CO3, calculate both the pH and the CO," ion concentration. -2 H2CO3 + H20 H;0" + HC03 Kal = 4.2x10-7 HCO3 + H2O=H30* {co,?- Ka2 = 4.8x10 11 pH = [Co,?) =
1. a. Tris (C4H6(OH)3NH2) has a Ka of 7.94 x 10−9. Calculate the Kbfor this compound. b. If a chemist was to make 50.0 mL 0.20 M solution of Tris, what would the pH be after an addition of 10.0 mL of 0.10 M HCl?
Solve question 5.
The acid ionization constant for Fe(H,O),*(aq) is 3.0x10-6. Calculate the pH of a 0.0170 M solution of Fe(NO3)2. pH =