A solution contains a mixture of 40 mL of 4.8 M HBr and 20 mL of 1.8 M NaOH. Calculate the pH of this solution. Please express your answer with two decimals. Hint 1: HBr(aq) + NaOH(aq) H2O() + NaBr(aq) Hint 2: HBr is a strong acid. NaOH is a strong base Hint 3: M=mol/L

A solution contains a mixture of 40 mL of 4.8 M HBr and 20 mL of 1.8 M NaOH. Calculate the pH of this solution. Please express your answer with two decimals. Hint 1: HBr(aq) + NaOH(aq) H2O() + NaBr(aq) Hint 2: HBr is a strong acid. NaOH is a strong base Hint 3: M=mol/L

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 is the pH of a solution that has pOH = (8.17x10^0)? Enter your answer in scientific notation…

Q: РОН 3D 10.8 1.4 x 104 М NaOH 3.1 х 10% М НСІ [Он] %3 1.1 х 10° М [н]3 2.0 х 10м

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: The strength of different acids can be compared on the basis of the degree of dissociation of these…

Q: Which of the following is the net ionic equation for the reaction that occurs when a few drops of…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: How do i set this question up.

A: Given:Mol. Of HCl = 0.0084Volume = 1500 mLMolarity of HCl =?Con. H3O+ = ?pH = ?

Q: Determine the pH of each of the following solutions. Give your answers to two decimal places of…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-¹ Ka(HCOOH) = 1.77 ×…

A: We know weak acids having lower value of dissociation constant Ka ionise weakly so can ignore their…

Q: Question 1 Calculate the pH of the resulting solution when 22.0 mL of 0.12 M KOH are added to 28.0…

A: In this question we have to tell the PH of the resulting solution.

Q: Indicate acids and bases 1) HCl(aq)= H+(Aq) + Cl- (aq) -I know HCl would be an acid, so would that…

A: This is acid base reaction.

Q: Consider sample of Sr(OH)2(aq) that was made by dissolving 0.239 g Sr(OH)2(s) in enough water to…

Q: Consider the following data on some weak acids and weak bases: name acid hydrofluoric acid HF…

A: The question is based on the concept of salt hydrolysis. We need to arrange given salts in…

Q: What is the pH of a solution that is 0.150 M NH3 and 0.200 M NH4CI? Kb of NH3 = 1.8 x 10-5 O9.26…

Q: Assuming equal concentrations, arrange these solutions by pH. Arrange from highest pH to lowest pH.…

Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL solution…

Q: You have a mixture of two weak acids, HF (Ka = 6.3 \ times 10^-4) and hypoiodous acid, HIO (Ka =…

A: To find the pH and [OH-] concentration in the given solution, we can use the Henderson-Hasselbalch…

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: The strength of different acids can be compared on the basis of the degree of dissociation of these…

Q: Ethanolamine, HOC₂H4NH₂, is a viscous liquid with an ammonia-like odor; it is used to remove…

A: Answer is given below in two part

Q: "Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which…

A: 1) Here given---- pH of the acid rain = 3.41 We know---- pH = - log [H+] Or, [H+] = 10-pH Now…

Q: The acid ionization constant for Al(H2O)63+(aq) is 7.9×10-6. Calculate the pH of a 0.0366 M solution…

A: Since you have posted multiple questions, the answer for first question is given below. Kindly…

Q: Calculate the value of [OH] from the given [H3O+] in Note: The ion product of water = 1.0 × 10¯¯ 14…

A: Part 1) .Given , [H3O+] = 10-6 M [OH-] = ? We know that, [H3O+] [OH-] = kw = 1.0×10-14 So, [OH-] =…

Q: You measured the pH of a 0.01M HCI solution (strong acid) and a 0.01M CH3COOH solution (weak acid).…

A: We know that is strong acid have almost 100% dissociation of hydronium ion and weak acid have nearly…

Q: What is the hydroxide ion, pH, and pOH of a solution with a hydrogen ion concentration of 3.25 x…

A: Given: [H+] = 3.25 x 10-3 M Kw = 10-14 Since [H+] < 10-7 M so solution is acidic in nature.…

Q: 1.209 g of strong base NaOH (molar mass 39.998 g/mol) is dissolved in enough water to make 6.65 L of…

Q: For each of the following substances, identify whether the substance is classified as an Arrhenius…

A: According to Arhenius , acid are the substance which release H+ ion and base are the substance…

Q: H2Z is a diprotic acid with Ka1 = 3.0 × 10^-3 and Ka2 = 8.0 x 10^-8. Suppose you start with 1.00 L…

A: The objective of the question is to determine the pH at the given volumes.It is given that,The…

Q: When you measured the pH of the 0.1M HCl solution, you placed 25mL of the solution in a 50mL beaker.…

A: The concentration of any chemical species, which is denoted by the square brackets, is given by the…

Q: In a system at equilibrium, the concentration of the NH3(aq) is 0.35 mol/L and the concentration of…

A: Concentration of NH3 = 0.35 MConcentration of NH4Cl = 0.25 MKa value of ammonia = 5.6*10-10pH =?

Q: When answering this problem, report the answer with the appropriate number of significant figures…

Q: sure your answer has the correct number of significant digits. Calculating the pH of a strong base…

A: Given : Mass of Barium hydroxide = 216. mg Volume of solution = 190. ml

Q: A student mixes 300 mL of 0.100 M NaOH with 100 mL of 0.300 M H,SO4. The resulting solution has a pH…

A: Given: The Volume of NaOH, (V1) = 300 mL The Volume of H2SO4, (V2) = 1 00 mL. The molarity of NaOH,…

Q: The pH of a white vinegar solution is 2.28. This vinegar is an aqueous solution of acetic acid with…

Q: A 0.245−mol sample of HX is dissolved in enough H2O to form 595.0 mL of solution. If the pH of the…

A: pH= 3.60

Q: What volume of a concentrated HCl solution, which is 36.0% HCI by mass and has a density of 1.179…

A: To determine the required volume of 36.0 % HCl solution to prepare the HCl solution of pH of 1.60,…

Q: Finding pH An unknown substance has a hydrogen ion concentration of 3H 4  3.1  108M. Find the pH…

A: Consider the hydrogen ion concentration of an unknown substance is [H+]= 3.1 x 10-8 M. The objective…

Q: For the reaction: HCO, (aq) + AsH(aq)=CO2(aq) + AsH¸* (aq) In order, these are best chategorized as…

A: If you have any help please let me know in comment box and then I will help you.

Q: Calculate the pH of the solution that results from mixing 74.0 mL of 0.061 MHCN(aq) with 26.0 mL of…

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: The strength of different acids can be compared on the basis of the degree of dissociation of these…

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

A solution contains a mixture of 40 mL of 4.8 M HBr and 20 mL of 1.8 M NaOH. Calculate the pH
of this solution. Please express your answer with two decimals.
Hint 1: HBr(aq) + NaOH(aq)
H2O(1) + NaBr(aq)
Hint 2: HBr is a strong acid. NaOH is a strong base
Hint 3: M-mol/L

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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 solution of HCl has a pH of 1.94. How many grams of HCl are there in 298 mL of this solution? g HCI How many grams of HCI are in 298 ml of a HCl solution that has twice the pH? g HCI
In a 1.00 M aqueous solution of sulfuric acid, H2SO4, three processes producing the hydronium ion is listed below. Which one do we have to consider if we are trying to calculate the pH of the solution? H2SO4 (aq) + H2O (l) --> H3O+ (aq) + HSO4- (aq) HSO4- (aq) + H2O (l) <-> H3O+ (aq) + SO42- (aq) Ka2 = 0.012 2 H2O (aq) <-> H3O+ (aq) + OH- (aq) Kw = 1.0 x 10-14
36. Which will have a lower (the lowest) pH among the solutions shown in each of the following questions? Justify your answers. a. 0.001 M NaOH and 0.005 M NaOH b. 0.001 M NaOH, 0.001 M NaCl, and 0.001 M HCI С. 0.001 M HCI and 0.001 M CH;COOH (acetic acid) d. 0.001 M NaOH and 0.001 M NH3 (ammonia)
The ionization of benzoic acid is represented by this equation. C6H5COOH(aq) ↔ H+(aq) + C6H5COO–(aq) If a 0.055 M solution of benzoic acid, at a certain temperature, has an [H+] =2.7 × l0−3, what is the Ka of benzoic acid?
Use the graph to show the change in concentration when: a persons blood pH change if they were taking part in strenuous activity or exercise? a persons blood pH change if they were hyperventelating ( breathing out more CO2 than normal?
ch1
Consider two solutions, solution A and solution B. [H+] in solution A is 450 times greater than that in solution B. What is the difference in the pHpH values of the two solutions? Express your answer using two decimal places. pH=
What is the pOH of (3.03x10^-1) M LIOH? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:
< Weak Acid HCN HNO HIO HBrO CH₂COOH + K₂ 4.9 x 10¹⁰ 4.5 x 10* 2.3 x 10¹¹ 2.5 x 10* 6.3 x 10° Which of the following 1.0 M solutions would have the lowest pH? Weak Base HONH, ΝΗ, CHÍNH, H,NNH, C.H.N Kb 1.1 x 10 1.8 x 10¹ Question 46 of 52 4.3 x 10.¹⁰ 1.3 x 10* 1.7 x 10° A) LINO, B) HONH,Br C) H₂NNH,CIO D) Ca(BrO)₂ ★ 10: Submit
Enough of a monoprotic weak acid is dissolved in water to produce a 0.0114 M solution. The pH of the resulting solution is 2.60. Calculate the K₂ for the acid. = K₂ = x10 TOOLS
Water ionizes by the equation Н20(1) — н+ (аq) + ОH (аq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H*] and [OH ]: Part A At a certain temperature, the pH of a neutral solution is 7.27. What is the value of Kw at that temperature? K, = [H*][OH¯] Express your answer numerically using two significant figures. Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. • View Available Hint(s) V ΑΣφ. ? Kw %3D Submit Part B What is the pH of a neutral solution at a temperature where Kw 9.9 x 10-14? Express your answer numerically using two decimal places. • View Available Hint(s) V ΑΣφ. pH = Submit
30 mL of 0.25 mol L' HNO3(aq) is placed in a flask and titrated with 0.25 mol L NaOH(aq) solution. What is the pH of the solution in the flask when 25 mL of the NaOH(aq) solution has been added? Answers A - D A 4.64 B 1.38 C 7.00 D 1.64