Answered: Which of the solutions listed below has…

Science

Chemistry

Which of the solutions listed below has the lowest pH? A. Pure H20 B. 2.5 x 10° M HNO3 C. 0.10 M NAOH D. 0.10 M HCI

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 31QRT: A 1000.-mL solution of hydrochloric acid has a pH of 1.3. Calculate the mass (g) of HCl dissolved in...

See similar textbooks

Related questions

Q: A chemist dissolves 451. mg of pure sodium hydroxide in enough water to make up 100. ml. of…

Q: what is the pH of a 0.235 M HNO3 solution? Report in 2 decimal places

Q: 105. Determine the pH of each solution. a. 0.10 M NH,CI c. 0.10 M NaCl b. 0.10 M NaC,H;Oz

Q: The pH of a solution is a measure of its acidity or alkalinity. Specifically, pH = -log[H+] where…

A: pH= -log[H+] Using this formula [H+] can be calculated.

Q: A chemist dissolves 130. mg of pure sodium hydroxide in enough water to make up 70. mL of solution.…

Q: A chemist dissolves 436. mg of pure barium hydroxide in enough water to make up 100. mL of solution.…

A: Given : Mass of barium hydroxide = 436 mg Volume of solution = 100. mL To calculate :- pH of…

Q: Calculate the pH of each solution.(a) [H3O+] = 1.7 * 10-8 M(b) [H3O+] = 1.0 * 10-7 M(c) [H3O+] = 2.2…

Q: A chemist dissolves 52. mg of pure sodium hydroxide in enough water to make up 60. mL of solution.…

Q: A chemist dissolves 213. mg of pure barium hydroxide in enough water to make up 130. mL of solution.…

A: pH of a solution is defined as the negative log of the hydrogen ion concentration. pOH of a solution…

Q: Which solution will have the lowest pH (most acidic)? a. 0.10 M HCIO. b. 0.10 М НСIO с. 0.10 МКОН d.…

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

Q: A chemist dissolves 670. mg of pure potassium hydroxide in enough water to make up 140. mL of…

Q: A chemist dissolves 600. mg of pure potassium hydroxide in enough water to make up 120. mL of…

A: Given:Mass of KOH =600mg =0.6gvolume of the solution, V=120mLTo find:pH of…

Q: A chemist dissolves 107. mg of pure potassium hydroxide in enough water to make up 70. mL of…

Q: A chemist dissolves 417. mg of pure potassium hydroxide in enough water to make up 160. mL of…

A: Applying concept of molarity and PH and POH. POH= -log [OH-]

Q: the pH of a mysterious solution has an H+ concentration of: 1.704 x 10-2 is. After finding the pH,…

Q: 2. Calculate the pH of each solution: (a) 0.0155 M HBr (b) 1.28 × 10-3 M KOH (c) 1.89 × 10-³ M HNO3…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: For which of the following solutions must we consider the ionization of water when calculating the…

Q: A chemist dissolves 622. mg of pure barium hydroxide in enough water to make up 180. mL of solution.…

Q: 6. Which solution has the highest pH? A. 0.10 M HCIO4 (aq) B. 0.10 M HBrO4 (aq) C. 0.10 MHCI0(aq) D.…

A: pH is defined as negative logarithm of hydrogen ions

Q: What is the pH of 0.174 M HNO3 solution

A: Given :- concentration of HNO3 Solution = 0.174 M To calculate :- pH of solution

Q: A chemist dissolves 212.mg of pure sodium hydroxide in enough water to make up 120.mL of solution.…

Q: Determine the pH of each solution. a. 0.0650 M HNO3 c. 0.0195 M KOH b. 0.150 M HNO2 d. 0.245 M…

A: Hi, since you have posted questions with multiple subparts. We will answer the first three subparts…

Q: Calculate the pH of a solution that has [H301 = 3.1 × 10-8 M. A) pH 3.18 B) pH = 3.10 C) pH 7.51 pH…

A: Answer

Q: A chemist dissolves 149. mg of pure potassium hydroxide in enough water to make up 110. mL of…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is simply…

Q: A chemist dissolves 601. mg of pure barium hydroxide in enough water too make up 100. mL of…

A: Given : Mass of Ba(OH)2 = 601 mg = 0.601 g…

Q: A chemist dissolves 325. mg of pure potassium hydroxide in enough water to make up 50. mL of…

Q: A chemist dissolves 203. mg of pure barium hydroxide in enough water to make up 60. mL of solution.…

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

Q: A chemist dissolves 890. mg of pure barium hydroxide in enough water to make up 110. mL of solution.…

A: Mass of barium hydroxide = 890 mg Volume of solution = 110 ml Temperature = 25 °C pH of the…

Q: A solution of HCl has a pH of 1.94. How many grams of HCl are there in 298 mL of this solution? g…

A: Given, the pH of HCl solution =1.94volume of soltuion =298 mL =0.298 Lwe are asked to calculate the…

Q: A chemist dissolves 601. mg of pure barium hydroxide in enough water to make up 190. mL of solution.…

Q: Calculate the pH of each solution: (a) 0.0155 M HBr (b) 1.28 × 10-³ M KOH (c) 1.89 × 10-3M HNO3 (d)…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

Q: A chemist dissolves 883. mg of pure sodium hydroxide in enough water to make up 60. mL of solution.…

Q: A chemist dissolves 121. mg of pure sodium hydroxide in enough water to make up 120. mL of solution.…

A: moles of NaOH dissolved = mass / molecular mass molecular mass of NaOH = 40 gm/mol Hence moles of…

Q: A chemist dissolves 339. mg of pure hydroiodic acid in enough water to make up 180. mL of solution.…

Q: Calculate the pH of each of the following strong acid solutions. A. 5.55×10−2 M HNO3. Express…

Q: A solution has an H3O+ concentration of 8.2 x 10-4M H3O+ What is the ph of this solution. Report…

A: Ph is a measurement of how acidic or basic a substance or solution is. pH is measured on a scale of…

Q: For a 0.40 M solution of HCIO4, calculate: [H+], pH, pOH, and [OH"] Determine all pH and pOH values…

Q: What is the pH of a 0.025 M solution of KOH?

Q: Calculate the pH of each solution. [H3O+] = 6.7×10−8 M [H3O+] = 7.0×10−7 M [H3O+] = 5.2×10−6 M…

A: The pH of the solution can be calculated by using the formula given below as; pH = - log H3O+…

Q: Which solution has the highest pH? A) 0.222 M HF B) 0.222 M HI C) 0.222 M HBr D) 0.222 M HClO4…

A: Acids are those compounds or molecules which liberate H+ ions in the aqueous solutions. Strong Acids…

Q: 794.mg of pure hydrobromic acid in enough water to make up 380.mL of solution. Calculate the pH

Q: A chemist dissolves 382. mg of pure sodium hydroxide in enough water to make up 70. mL of solution.…

A: Solution : We need to calculate the molarity of the solution first 1M NaOH=40g of NaOH in 1 L of…

Q: Which solution is most likely to result in a solution with a neutral pH? O a. Zn(NO3)2(aq) O b.…

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

Q: A chemist dissolves 87. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

Q: 1. Which solution has the lowest pH? A. 0.10 M HCIO, В. О.10 М НСО C. 0.10 M KOH D. 0.10 M CH,NH;

A: The pH of the solution depends upon the negative logarithm of hydrogen ion concentration and written…

Q: A chemist dissolves 98. mg of pure barium hydroxide in enough water to make up 80. mL of solution.…

Q: A 0.365g sample of HCI is dissolved in enough water to give 2.00 x 10-2 ml of solution. What is the…

Q: certain weak base has a ?b of 7.80×10−7. What concentration of this base will produce a pH of…

Q: Calculate the pH of ... ... 2.00 L of a 12.1 M HCl solution.

A: Given :- 2.00 L of 12.1 M HCl We have to calculate the pH of this solution. pH = - log [H+] ion. As…

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

Which of the solutions listed below has the lowest pH?
A. Pure H20
B. 2.5 x 10 M HNO;
C. 0.10 M NAOH
D. 0.10 M HCI

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

Step 2

Step 3

Step 4

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

A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?
A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of solution. The pH of the final solution is 4.56. a What is the molar concentration of the acetic acid? b How many milliliters of hydrochloric acid were added to the original solution? c What was the original concentration of the sodium acetate?
What volume of 0.120 M NaOH must be added to 100. mL of 0.100 M NaHC2O4 to reach a pH of 4.70?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.
A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a Write the net ionic equation that represents the reaction of this solution with a strong acid. b Write the net ionic equation that represents the reaction of this solution with a strong base. c To 100. mL of this solution, 10.0 mL of 1.00 M HCl is added. How many moles of NH3 and NH4+ are present in the reaction system before and after the addition of the HCl? What is the pH of the resulting solution? d Why did the pH change only slightly upon the addition of HCl?
A 1000.-mL solution of hydrochloric acid has a pH of 1.3. Calculate the mass (g) of HCl dissolved in the solution.
A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the following statements is most likely to be correct? a The pH of the solution at the equivalence point is 7.0. b The pH of the solution is greater than 13.0. c The pH of the solution is less than 2.0. d The pH of the solution is between 2.0 and 7.0. e The pH of the solution is between 7.0 and 13.0. The reason that best supports my choosing the answer above is a Whenever a solution is titrated with a strong acid, the solution will be very acidic. b Because the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. c Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidic.
Sodium benzoate, NaC7H5O2, is used as a preservative in foods. Consider a 50.0-mL sample of 0.250 M NaC7H5O2 being titrated by 0.200 M HBr. Calculate the pH of the solution: a when no HBr has been added; b after the addition of 50.0 mL of the HBr solution; c at the equivalence point; d after the addition of 75.00 mL of the HBr solution. The Kb value for the benzoate ion is 1.6 1010.
A solution of KOH has a pH of 13.29. It requires 27.66 mL of 0.2500 M HCI to reach the equivalence point. (a) What is the volume of the KOH solution? (b) What is the pH at the equivalence point? (c) What is [K+] and [Cl-] at the equivalence point? Assume volumes are additive.
Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCI. A 75.00-mL sample of the diluted solution is titrated to pH 7.00 with 78.8 mL of 4.85 M NaOH. How much water was accidentally added? (Assume that volumes are additive.)
An important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?