How many grams of NH:Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? TheKb of NH3 is equal to 1.8 x 10-5.123NEXT>Let x represent the original concentration of NH4* in the water. Based on the given values, set up the ICE table in order todetermine the unknown.NH: (aq)H:O(1)H:O“(aq)NH:(aq)++Initial (M)Change (M)Equilibrium (M)5 RESET1.005.161.8 x 1052x0.5x-2x-0.5x6.9 x 10-6.9 x 1060.709-0.709x + 6.9 x 10-x- 6.9 x 10-x+ 0.709X - 0.709

Given that, pH of the solution = 5.16 Kb of NH3 = 1.8×10-5 Now, we have to calculate the amount of…

Answered: How many grams of NH:Br must be…

How many grams of NH:Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NHs is equal to 1.8 × 10-5.

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: Ka for HOCl is 3.2 × 10-8. How much chlorine (g) must be dissolved in 2.0 liter of water so that…

A: Given data are as follows Chemical reaction Cl2(g) + H2O(l) ⇌ H+(aq) + Cl–(aq) + HOCl(aq) Ka for…

Q: How many moles of NH3 must be dissolved in water to give 665.4 mL of solution with a pH of 11.01? Ko…

Q: Consider the following data on some weak acids and weak bases: acid base K. K, name formula name…

A: We have to predict the order of pH of solution.

Q: OH,O and H,PO OH,PO, and H,PO O HO and H,PO OH,PO, and OH 7) The conjugate base of NH," is OH. O…

A: •This question is based on conjugate acid and base. •So firstly we understand about conjugate acid…

Q: What is the pH of a 0.24 M solution of sodium propionate, NaC3H5O2, (base) at 25°C? (For propionic…

Q: Calculate the pH of a 4.80×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid,…

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

Q: Calculate the pH of a solution that is prepared by diluting 0.140 moles of sodium benzoate to 1.00…

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: Bleach is a solution of sodium hypochlorite (NaClO). If 3.104 mol of NaClO is dissolved in 423 L of…

Q: Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the…

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

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

A: NaClO is salt made by strong base sodium hydroxide and weak acid HClO

Q: [H;O1+] 9.84 x 109M

Q: Consider the following data on some weak acids and weak bases: acid base K. K3 name formula name…

Q: pH and pOH of [H+] = 7.23×10-4 M

A: Given : [H+ ] = 7.23 X 10-4 M

Q: Calculate the [H3O+], [OH-], pH and pOH of a 0.120 M HNO2 (nitrous acid). Ka = 7.10 x 10-4

A: pH of a solution is given by the negative logarithm of hydrogen ion concentration in the solution…

Q: A 0.60 M solution of a weak acid, HA, has a pH of 3.41. What is the percentage ionization of the…

A: ★ Answer : percentage of ionization of the acid is 0.064%

Q: Part A If 15.0 mL of glacial acetic acid (pure HC2H3O2; K₂ = 1.8 × 10−5) is diluted to 1.70 L with…

Q: Morphine, C 17H 19NO 3, is often used to control severe post-operative pain. What is the pH of the…

A: Which one of the following is correct answer

Q: What is the pH of a 0.16 M solution of methylammonium chloride, CH;NH; Cl? What is the concentration…

Q: What the pH of a solution containing [H3O+] = 5.62 x 10-11 mol L-1 ?

A: Given that, for a solution [H3O+] = 5.62×10-11 mol/L. We have to calculate the pH of the solution.

Q: What quantity of moles of glucose (C₆H₁₂O₆) in 0.500 L of a 0.400 M solutions? The pH of a basic…

Q: Consider a 1.0 L of 0.1 M aqueous solution consisting of weak acid HA, which has K₂ = 3.9 x 10-4, at…

A: HA is a weak acid that is very weakly dissociated to give H+(aq) ions. HCl is a very strong acid…

Q: Calculate the pH of a solution that is made by dissolving 5.54 g NH4NO3 in enough water to create…

A: First to calculate morality Then to calculate degree of dissociation. Then to calculate pH.

Q: What is the pH of a 3.1 x 10-4 M CsOH solution?

A: Given : concentration of CsOH = 3.1 × 10-4 M To calculate :- pH of solution

Q: 10. How many moles of solid NaOH must be added to 1.0 L of 2.0 M HCl solution to reach a [OH] = 1.0…

A: To find out how many moles of solid NaOH must be added to the HCl solution to reach a hydroxide ion…

Q: Determine the pH of a solution that is prepared by dissolving 7.2 g of Ba(OH)2 in 4.7 L water at…

A: 1. Molarity of Ba(OH)2 : number of moles of solute (n) in 1 L solution is called molarity (M) M…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: Answer:- This question is answered by using the simple concept of calculation of weak acid and the…

Q: What is the pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

A: Given, The pH of a solution prepared by dissolving 0.450 mol of NH3 in sufficient water to make…

Q: Which would you expect to be the better Lewis base, C^4- or Si^4-? Explain.

A: Species which can donate electron/s or electron density is called lewis base. And electron donation…

Q: Unit 2: Chemical Systems & Equilibrium Butanoic acid, C3H₂COOH, gives rancid butter its distinctive…

Q: Calculate the pH of a 0.175 M solution of aqueous ammonia. Kb = 1.8 x 10-5

A: Write the equilibrium expression for the base dissociation of ammonia:NH3+H2O⇌NH4++OH− Write the…

Q: Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86. Round to…

Q: What is the pH of an aqueous 0.25 M NaBrO solution? Ka(HBrO) = 2.0 × 10-9

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

How many grams of NH:Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The
Kb of NH3 is equal to 1.8 x 10-5.
1
2
3
NEXT
>
Let x represent the original concentration of NH4* in the water. Based on the given values, set up the ICE table in order to
determine the unknown.
NH: (aq)
H:O(1)
H:O“(aq)
NH:(aq)
+
+
Initial (M)
Change (M)
Equilibrium (M)
5 RESET
1.00
5.16
1.8 x 105
2x
0.5x
-2x
-0.5x
6.9 x 10
-6.9 x 106
0.709
-0.709
x + 6.9 x 10-
x- 6.9 x 10-
x+ 0.709
X - 0.709

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

Calculate the pH of a solution that is 1.8*10^-3 M morphine if the pKa of its conjugate acid is 8.21
Calculate the ph of a solution that is prepared by dissolving 8.57 NaC2H3O2(82.03g/mol) in enough water to make 0.477L of solution. The Ka of HC2H3O2 is 1.8 x 10-5
what is the ph of a 0.81 M hypochlorous acid (HClO) solution? Ka=3.0x10-8 for the acid.
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 ).
What mass of NAOH(s) must be added to 1.0 L of 0.072 M NH3 to ensure that the percent ionization of NH3 is no greater than 0.0014%? Assume no volume change on addition of NaOH. (K, for NH3 is 1.8 x 10-.) Mass =
Which ionic molecule acts as a stronger base and why? CH;CH vs CHC
5. solution is acidic or basic. Make the following conversions. Report answers to 2 decimal places.In each case, tell whether the pH 10.61 [H,O'] [ОН] acidic or basic? (b) 1.76 x 106 2.45 x 10-11
Aluminum has been implicated as a neurotoxic agent for Alzheimer’s patients and is known as harmful for renal failure patients. In 1985, the medical community recommended that no more than 10 mg/L Al3+ be present in drinking water used for dialysis patients. At what pH is the maximum Al3+ concentration equal to 10 mg/L, assuming that the only source of Al3+ is Al(OH)3? How does this compare with the allowable pH of drinking water of 7.8; would we expect to observe this concentration in drinking water?
Consider the following data on some weak acids and weak bases: acid base K K, name formula name formula - 10 hydrocyanic acid HCN |4.9 × 10 methylamine CH3NH2 |4.4 x 10 HNO, 4.5 x 10¯* 8. nitrous acid hydroxylamine HONH, 1.1 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М КBr v choose one D 1 (lowest) 0.1 М HONH3CІ 2 3 0.1 М CН3NH3Br 4 (highest) 0.1 М КCN choose one
Calculate the pH of an aqueous KOH solution that is made by dissolving 654 mg of solid KOH in enough distilled water to make 100.0 mL of solution. Assume room temperature conditions. Note: molar mass of KOH = 56.105 g/mol; Kw at 25 °C = 1.00 × 10-14 %3D %D 6.987 10.000 0.933 13.066
What is the pH of a solution created by combining 1.13 mole of HOBr and 0.49 mole NaOH in a 1.00L solution? Ka HOBr = 2.5 x 10-9
Calculate the pH of a solution made by dissolving 0.0100 mol of NH3 in enough water to give 1.000 L of solution at 25 oC. The Kb for ammonia is 1.8 x 10-5.