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: What mass ofn HNO3 is present in 285.0 mL of a nitric acid solution having a pH of 4.39? Mass =…

A: The answer to the following question is- Given, Volume of solution = 285 mL pH= 4.39

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: What is the pH of a 0.0380 M solution of HONH CI (Kb of HONH₂ is 1.1 x 10°)?

A: The pH of any acidic mixture is always low.

Q: A solution is made by dissolving 13.9 g of HONH:CIO3 in 500.0 mL of water. Does CIOS- have any…

Q: What is the pH of a 0.785 M solution of formic acid, HCHO2? The Ka of HCHO2 is 1.77 x 10-4.

A: In an aqueous solution of HCHO2, the dissociation of weak acid HCHO2 and autoionization of water…

Q: A chemist dissolves 830. mg of pure hydrobromic acid in enough water to make up 300. mL of solution.…

A: pH = 1.466 Explanation:Given mass of hydrobromic acid = 830. mg or 830 mg/1000 mg/g = 0.830…

Q: 6) Explain why a 0.010 M solution of hydrochloric acid, HCl has a pH of 2.00 but a 0.010 M solution…

Q: Household bleach is prepared by dissolving chlorine in water. Cl2(g) + H2O(l) ⇌ H+(aq) + Cl–(aq) +…

A: Given information: Ka for HOCl = 3.2 × 10-8 Volume of water = 3 litres. PH = 2.51 Given equation:…

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: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

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: HA is a weak acid. Its dissociation constant, Ka, is 2.2 x 10-13. What is the pH of an aqueous…

Q: Aspirin is acetylsalicylic acid, HC,H,O4, which has a K, of 3.0 × 10¬4. Calculate the pH of a…

A: Given information: Mass of acetylsalicylic acid = 0.65 g Volume = 50.0 mL

Q: NH3 is a weak base (K₁ = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: A solution is given that is 0.036 M in NH4Cl at 25oCKb = 1.8*10-5Need to find the pH

Q: How many moles of NH4Cl must be dissolved in 500. mL of aqueous solution, in order to produce a…

Q: What molar concentration of hydrazine, N2H4 (Kb = 1.7 x 10^-6) yields a solution with a pH of10.46?

A: The objective of this question is to find the molar concentration of hydrazine, N2H4 that yields a…

Q: What is the pH of a 0.430 M solution of CH NHBr (Kb of CHN is 1.7 × 10º)?

A: Given information:Calculate pH. .pH is the measurement of acidity or alkalinity of solution. A…

Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3? The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: the pH of a 100mL buffer solution containing 0M HC2H3O2 and 1.0M NaC2H3O2 after 30mL of 1.0M NaOH…

A: Given question is based upon acidic buffer . So we will use Henderson-Hasselbalch equation.

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: We place 0.586 mol of a weak acid, HA, and 12.6 g of NaOH in enough water to produce 1.00 L of…

A: Step 1: Step 2: Step 3: Step 4:

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

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: A chemist dissolves 643. mg of pure perchloric acid in enough water to make up 250. mL of solution.…

A: Given, mass of perchloric acid = 643 mg = 0.643 g…

Q: 1--The solution of substance (X) is completely ionized in water, its pH value is (10), so its…

A: Dear student , since you have posted multiple questions we are allowed to solve only first question…

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: Can you please answer question 5

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Milk of magnesia is a suspension of magnesium hydroxide in water. Although Mg(OH)2 is relatively…

A: given, pH of solution = 10.08

Q: Household bleach is prepared by dissolving chlorine in water. Cl2 (g) + H2O « H+ (aq) + Cl-…

A: The hydrogen ion concentration in the solution of a pH of 1.19 is;

Q: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…

A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…

Q: what is the pH of a solution containing 7.1 g of acetic acid (HC2H3O2) dissolved in 240 mL of water?…

A: Acetic acid i.e CH3COOH is a weak monoprotic acid. Hence it will dissociate partially in the…

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 7.9 g of Ba(OH)2 in 1.9 L water at…

A: Molar mass of Ba = 137.3g/mol Molar mass of O = 16.00g/mol Molar mass of H = 1.008g/mol

Q: HA is a weak acid. Its ionization constant, Ka, is 2.4 x 10-13. Calculate the pH of an aqueous…

A: Given : The solution has salt NaA with concentration 0.063 M Since NaA is an ionic salt. Hence it…

Q: calculate the pH and pOH of a 4.3 x10-3M solution of NaOH

A: Concentration of NaOH = 4.3 x 10-3M NaOH is a strong base and it can dissociate into its ions…

Q: If you mix 11.5 grams of HNO3 into 10.26 liters of water, what is the pH? How many grams of Acetic…

A: Given data,Mass of HNO3=11.5gVolume of water=10.26L

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

HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NACIO acts as a weak base. What is the pH of a solution that is 0.033 M in NaCIO at 25 °C? pH =
1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.061 M. 2.) We place 0.149 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.11 . Calculate the ionization contant, Ka, of HA. 3.)We place 0.527 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.35 . Calculate the ionization constant, Ka, of HA.
The pH of a 0.05 M NaOH solution at 25 °C is: O 13.8 O 13.1 O 11.5 • 12.7 O 10.3
What is the pH of a 0.320 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?
Determine the pH of a solution that is prepared by dissolving 8.6 g of Ba(OH)2 in 1.3 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.
What is the pH of a 0.785M solution of formic acid,HCHO2?The Ka of HCHO2 is 1.77x10-4?
Unit 2: Chemical Systems & Equilibrium Butanoic acid, C3H₂COOH, gives rancid butter its distinctive odour. Calculate the pH of 0.020 mol/L solution of butanoic acid. K₂ = 1.51 x 10-5
What is the concentration of hydroxide ion in a 0.76 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 10-14.) what is M ? What is the pH ?
Calculate the pH of a 0.175 M solution of aqueous ammonia. Kb = 1.8 x 10-5
Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86. Round to one decimal place.
Calculate the pH of the amphiprotic salt NaHA. Ka (H2A) = 0.0026, Ka (HA-) = 0.0000000077
6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a pH of 2.44? Note that the Ka of benzoic acid is 6.3 x 10°.