Answered: 5) if 125.0 ml water is added to 175.0…

5) if 125.0 ml water is added to 175.0 ml a strong acid solution of PH = 3. What should be the PH of the solution after dilution (M, x V. = Ma x Va)? a) 1.75 b) 3.23 c) 2.85

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 9RQ: What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a...

See similar textbooks

Related questions

Q: • Calculate the pH of water sample with hydrogen ion concentration of 3.16 * 10-8 mols/L • Calculate…

A: pH = - log [H+]

Q: A.1. Write the phrase to establish equilibrium. A.2. Calculate the pH of the propanoic acid…

A: Propanoic acid reacts with water to form propanoate ion and hydronium ion.…

Q: What is the pH if the Kb for NH3 is 1.8x10-5?

A: pOH +pH = 14 So, pH = 14 - pOH Initially we find the pOH with the help of Henderson-Hasselbalch…

Q: What is the hydroxide-ion molarity in an aqueous solution at 25 °C that has a pH value of pH =6.10?…

Q: Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4…

A: Given- Concentration of CH3NH2 = 0.35 M Kb = 4.4 × 10-4 To find - pH of solution Formula- pH = - log…

Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…

A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…

Q: What is the resulting pH of a solution at 298 K made by mixing 50.0 mL of 0.355 M HCl and 25.0 mL of…

Q: What is the pH of a 0.220 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?

A: Aniline is a weak base. C6H5NH2+H2O⇔C6H5NH3++OH- 1 0…

Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,l? (Kb of CH;NH, is 4.4 x…

A: This is a basic buffer solution. A buffer resist the change in PH of the solution.

Q: A 1.00 L solution contains benzoic acid (C7 H5 O₂ H) with a concentration of 0.250 mol/L,and sodium…

Q: What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate base…

A: The solution is given below -

Q: What mass (in g) of potassium fluoride should be added to 0.50 Lof 0.255-M HF(aq) at 25 °C to give a…

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

A: Kw = Ka x Kb Kw = 1x10-14 given that Ka = 4x10-8 find Kb = (1x10-14) / (4x10-8) = 2.5x10-7 Initial…

Q: Calculate the mass of solid NaCH3CO0 that must be added to 1.0 liter of 0.20 M CH3COOH solution so…

Q: Ascorbic acid (vitamin C, C6H8O6, 176.1256 g/mol ) is a water soluble vitamin. A solution contains…

A: Molarity - It is calculated as moles of solute dissolved per liter of solution. The pH of weak…

Q: For a 0.0359 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What…

A: The chemical equation showing the ionization of cyanic acid is represented as follows:

Q: What is the pH of the solution obtained when 130 mL of 0.610 M NaOH is diluted to 16.0 L with water?…

A: Given: Initial concentration of NaOH = 0.610 M Initial volume of solution = 130 mL = 0.130 L…

Q: 5. At 25°C, what changes in pH occur when (a) 0.0250 M HCI (b) 0.0250 M NaOH are diluted with water…

A: We have to predict the change in the pH.

Q: 1. Which of the household solutions tested are acids? How can you tell? 2. Which of the solutions…

Q: Dilution. 100 mL100 mL of a solution of hydrochloric acid with pH 5.0 pH 5.0 is diluted to 1 L1 L.…

A: pH of a solution is equal to the negative logarithm of hydrogen ion concentration. Using this…

Q: 1.What is the percent relative uncertainty of pH of a 0.1861(±0.0004) molar solution of HCl?…

A: Interpretation- To determine percent relative uncertainty of pH of 0.1861(±0.0004) molar solution…

Q: Calculate the ph of a solution that is made by dissolving 6.45g of NH4Cl(53.49g/mol) in enough water…

A: First calculate molarity by mole/volume. Then use weak base concept to get pH

Q: How many grams of benzoic acid (CH:CO2H, 122.12 g mol", K = 63×10-7) is rquired t prepare an aqueous…

Q: Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine…

Q: How many milliliters of 0.800 M KOH should be added to 3.38 g of oxalic acid (C2O4H2) to give a pH…

A: Reaction: H2Ox + OH- —->HOx- + H2OHOx- + OH- ——->Ox- + H2O Equilibrium: H2Ox ——>HOx- + H…

Q: If K, is 2.9 x 10-15 -15 at 10°C, what is the pH of pure water at ?10°C 7.27 7.53 O 5.72 7.00

A: Given : Kw = 2.9 X 10-15 at 10oC Kw is the ionisation constant or equilibrium constant of the…

Q: a value of 7.2 x 10*. What is the pH to 2 decimal -f hydrofluoric acid with a concentration of 0.537…

A: We will calculate pH

Q: Orthocresol (C7H8OH) has a Ka - 5.50 x 1011. if 100.0 mL of a 0.5000 M aqueous orthocresol solution…

A: Write the acid dissociation of orthocresol in aqueous medium: C7 H8OH (aq)+H2O(l)→C7 H8O-(aq) + H3O…

Q: What is the expected pH of an aqueous solution consisting 150.0 mL 0.2500 M HBr04 mixed with 150.0…

Q: In the laboratory, a general chemistry student measured the pH of a 0.400 M aqueous solution of…

A: To find Kb for base, first write reaction of base with water and according to that, find [OH-] or…

Q: Normally, the volume of gastric acid in the human stomach ranges from 20. mL to 100. mL and a pH…

A: Given: Volume of the solution= 20 mL to 100 mL The given pH range =1.5 to 3.5 For the minimum…

Q: Which of the following 1.25M aqueous solution will have the lowest pH? (Qualitative analysis only,…

A: Concentration = 1.25 M ->Base has pH greater than 7. ->Acids has pH less than 7. ->Neutral…

Q: Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.

Q: 5.55 grams of solid calcium chloride, CaCl2, was dissolve in 250 mL of water to make a CaCl2…

A: given: mass = 5.5 g molar mass of CaCl2 = 110.98 volume = 250 mL = 0.25 L pH = ?

Q: Calculate the pH of a weak base which dissociates as BOH ⇌ B+ + OH- ( like NH3 (g) + H2O(l) →…

A: The dissociation reaction taking place is BOH ⇌ B+ + OH-

Q: A 46.2 cm3 volume of 0.00020 mol / dm3 barium hydroxide solution and a 27.0 cm3 volume of 0.100 mol…

A: Given: The volume of 0.00020 mol/dm3 barium hydroxide (Ba(OH)2) used is 46.2 cm3. The volume of…

Q: Trimethylamine, (CH3)3NH2, is a gas with a fishy, ammonialike odor. A 0.25 M aqueous solution of…

A: Since you have posted multiple questions, we are entitled to answer the first only. NOTE : The…

Q: The pH of a 0.016 M aqueous solution of p-toluidine (CH3C6H4NH2) is 8.60. Calculate Kb.

A: Concentration of OH- ions can be determined as follows,

Q: Determine the pH and the type of solution of a 0.227 g/L C5H5N solution at 25°C. The Kb of C5H5N is…

A: At 25°C Concentration=0.227g/L Kb of C5H5N = 1.7 ×10^-9

Q: What is the pH of 0.075 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 × 10−4.)

A: The value of Kb for the given weak base methylammonium bromide is = 4.4x10-4 The concentration of…

Q: What is the pH of a solution made from combining 6.56 mol C6H5NH3Cl and 7.58 mol C6H5NH2 in a 4.37 L…

A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…

Q: Kb for NH3 is 1.8 × 10-5. What is the pH of a 0.45 M aqueous solution of NH4Cl at 25.0 °C? Show

A: This question is related to salt hydrolysis of salt. By applying certain formula for that, required…

Q: calculate the pu aba 0-253M NH3 solution. NH3 has a Kb = 1.8 X 10^ _ 5. PH = ?

Q: Referencen) What volume of 0.0830 M NaOH must be added to 100. mL of 0.100 M NAHC0, to reach a pH of…

A: Volume of NaOH needed can be calculated from the Henderson hasselbalch equation the concentration of…

Q: What is the pH of a solution made by mixing 2.222 grams of benzoic acid, C6H5COOH with 150. mL of…

A: The given volume is 150 mL.It is known that, 1 mL = 0.001 L.Therefore, 150 mL = 0.15 L The mass of…

Q: In the laboratory, a general chemistry student measured the pH of a 0.423 M aqueous solution of…

A: The value of Kb for the given weak base is = 7.3x10-6 The concentration of the base solution is =…

Q: What is the expected pH of a 150.0 mL 0.250 M solution of HOCI which is diluted to a 500.0 ml mark…

A: Given that, a 150.0 mL of 0.250 M solution of HOCl is diluted to 500.0 mL, i.e., V1 = 150.0 mL, S1 =…

Q: Hydroxylamine, HONH2, readily forms salts such as hydroxylamine hydrochloride which are used as…

A: Since Kb of hydroxylamine is very less so it is assumed that reaction proceeds upto very less extent…

Q: A solution of 0.05 M benzoic acid (C6H5COOH) and 0.10 M sodium benzoate (C6H5COONa) has a pH of 4.50…

A: The above-given problem can be solved using the Henderson-Hesselbalch equation. pH = pKa +…

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

5) if 125.0 ml water is added to 175.0 ml a strong acid solution of PH = 3. What should be the PH of the
solution after dilution (M, x V. = Ma x Va)?
a) 1.75
b) 3.23
c) 2.85

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3 Calculating the Molarity before dilution

VIEW

Step 4

VIEW

Step by step

Solved in 4 steps with 3 images

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

Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 175 mL of a buffer that is 0.460 M in both propanoic acid (C,H,COOH) and its conjugate base (C,H,CO0-). Calculate the maximum volume of 0.380 M HCl that can be added to the buffer before its buffering capacity is lost.
4 a) Calculate the pH of the solution formed when 100 cm³ of 0.100 mol dm³ H₂SO4 is added to 50 cm³ of 0.500 mol dm NaOH. b) Calculate the pH of the solution formed when 25 cm³ of 0.250 mol dm³ HCI is added to 15 cm³ of 0.100 mol dm KOH. 5 Calculate the pH of the solution formed when 3.5 g of impure sodium hydroxide (98.7 % purity) is dissolved in water and made up to 100 cm³, and then 25 cm³ of 0.35 mol dm³ diprotic acid is added.
A solution of volume 0.500 L contains 1.68 g NH3 (Kb = 1.8 x 10^-5) and 4.05 g (NH4)2SO4. How many milliliters of 12 M HCI must be added to 0.500 K of the original solution to change its pH to 9.00?
Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) (a no KOH added???? (b)20. mL of KOH solution added???? (c)39 mL of KOH solution added???? (d)40. mL of KOH solution added???? (e)41 mL of KOH solution added????
You have75.0 mL of a 0.25M solution of a weak base, ethanol amine, HOC2H4NH2, with a kb= 2.8x10^-5. It is to be titrated with 0.50 M HCl. What is the pH of the resulting solutions after the following additions? (a) initial pH (B)after 10.50 mL of HCl have been added (c) 1/2 way to the equivalence point (d) at the equivalence point (E) after 40 mL of HCl has been added (f) what indicator would you choose to signal the endpoint, and WHY?
A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of propanoic acid (HPr, K«= 1.3 x 10-5). Assume the volume of the solution to be 1.0 L. a) Write the chemical equation for the acid hydrolysis reaction. | b) What is the acid-base conjugate pair that governs the pH of the buffer? c) Calculate the pH of the buffer. Be sure to justify and validate any approximations used.
You are asked to prepare a pH = 4.00 buffer startingfrom 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and any amount you need of sodium benzoate(C6H5COONa). (a) What is the pH of the benzoic acidsolution prior to adding sodium benzoate? (b) How manygrams of sodium benzoate should be added to prepare thebuffer? Neglect the small volume change that occurs whenthe sodium benzoate is added.