A solution is prepared by mixing 2.3 x 104 moles of sodium hydroxide (NaOH) and 4.5 x 10-6 moles of hydrobromic acid (HBr). Water (H,O) was added until the volume was 1.00 L. What is the pH of this solution? a. 9.86 b. 10.21 C. 10.35 d. 11.55

A solution is prepared by mixing 2.3 x 104 moles of sodium hydroxide (NaOH) and 4.5 x 10-6 moles of hydrobromic acid (HBr). Water (H,O) was added until the volume was 1.00 L. What is the pH of this solution? a. 9.86 b. 10.21 C. 10.35 d. 11.55

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: The following question refers to the following system: A 1.0 liter solution contains 0.25 M HF and…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: 2. H₂SO4 solution is prepared by dissolving 4.9 grams of H₂SO4 in 100 mL of water. many H₂SO4…

Q: . Which of the following solutions the has the lowest pH? A. 0.50 M HNO₂ (Ka = 4.6 x 10-4) B. 5.00 M…

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

Q: 11. The pH of a Ba(OH)2 solution is 10.00. What is the Ht ion concentration of this solution? A. 4.0…

A: pH is used to determine the concentration of hydronium ion.

Q: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

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

Q: If you have 0.80 g of solid KOH dissolved in 2.28 L of water: a. Determine the concentration of H…

A: Given Mass of Solid KOH (W) = 0.80g Molar mass Of KOH = 56.10 g/mol Number of moles dissolved (n)…

Q: 15. Calculate the pH of a 0.10 M NH4CN solution 16. Calculate the pH of a solution prepared by…

A: The pH of a solution is a measure of its acidity or basicity. It is defined as the negative…

Q: Consider two solutions: solution X has a pH of 5; solution Y has a pH of 7. From this information,…

Q: A solution is made by dissolving 0.0015 mole Ba(OH)2 in enough water to make 1.50 liter of solution.…

A: dExplanation:

Q: The pH of an aqueous solution at 25.0 °C is 10.20. What is the molarity of H+ in this solution? A.…

A: pH = -log[H+] 10.20 = -log[H+] [H+]=10-10.22 = 6.30×10-11 M

Q: A sample of water from the Chesapeake Bay has [H3O+] = 3.1 x 10-6 M. Which statement below…

Q: 38. Fluorinating water is traditionally done to protect the enamel on teeth. One method used to…

Q: 5.12

A: PH

Q: 27. If exactly equal mole amounts of KOH and HCl are reacted in a pure water solution, what will be…

A: The balanced chemical equation for the chemical reaction between KOH and HCl can be written as…

Q: Pre-Lab Q Vinegar is a common substance found in many kitchens. Predict whether vinegar is an acid…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: This compound is a weak organic base: C18H21O3N + H2O C18H21O3NH+ + OH-…

Q: 7) 150.0 mL of 2.50 M NaOH is added to a 200.0 mL solution of 1.80 M HF. Assume that the volumes are…

A: HF + NaOH→ NaF + H2O1.80M 2.50M200ml 150mlno. of moles of…

Q: 9. Which of the following solutions for a weak acid at equilibrium would have the largest pH? d. 3.2…

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

Q: A 4.0 M HCl solution is used to titrate a 2.0 M KOH solution. a. How many ml of the HCl…

A: To solve the question regarding neutralization reaction.

Q: If a solution of aspirin has a [OH-] = 4.4 x 10–12 M, what is the pH of the solution?

A: Given, [OH-] = 4.4 ×10-12 pH is the negative logarithm in hydrogen ion concentration.

Q: A.) The hydronium ion concentration in an aqueous solution at 25°C is 5.2×10-2 M. The hydroxide ion…

Q: Identify the major species present in each solution. The strongest acid will react with the…

A: 0.12 M KNO2 b. 0.45 M NaOCl c. 0.40 M NH4ClO4

Q: 10. What is the hydrogen ion concentration of a solution with a pH of 10.33? d. 4.68 X 10-4 e. 2.14…

A: The objective of this question is to calculate the hydrogen ion concentration of a solution given…

Q: A solution containing 2.60 x 10-3 moles of HCl and 3.32 x 10-3 moles of NaOH into a container and…

A: Given:- For a solution in a container, No of moles of HCl = 2.60 x 10-3 No of moles of NaOH = 3.32…

Q: The concentration of H+ ions in a solution is 0.315 M. a. Calculate the concentration of OH– ions…

A: Applying formula PH= -log[H+]

Q: 1.0 x 10-11 moles of HCl are added to 1.OL of H20. What is the pH? О 3.0 O 10.0 O 11.0 О 1.0 O 7.0

A: Moles of HCl = 1.0 × 10-11 moles Volume of water = 1.0 Liter

Q: 1. For each hydronium ion concentration, determine the hydroxide ion concentration and for each…

A: The formula to find hydroxide ion concentration is:The formula to find hydronium ion concentration…

Q: 22. Hydrochloric acid (HCI) is a strong acid, and Hydroiodic acid (HI) is a weak acid. Which of the…

A: Introduction: As per Bronsted-Lowry concept, an acid is a substance that can donate H+ ions and base…

Q: The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10. What is the pH…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: What is the pH of a solution made by mixing 40.0 mL of 0.20 M HCl with 40.0 mL of 0.10 M KOH?…

A: HCl and KOH will react as per the following reaction HCl + KOH --> KCl + H2O

Q: One aqueous solution of a strong acid has pH = 1.20, another pH = 1.80. If equal volumes of these…

A: First find the H+ concentration of both the solutions and find H+ concentration after mixing the…

Q: pOH

Q: a. A solution of HNO3 has a pH of 3.69. What is the molarity of the solution? Molarity |M b. A…

A: We know that, HNO3 is strong acid. So, it is completely dissociated. Thus, pH= -log[H+] Thus, [H+]…

Q: A solution is prepared by mixing 10mL of 1 M HCI and 10mL of 1.2 M NaOH. What is the pH of the…

Q: a. A solution of HINO, has a pH of 3.57. What is the molarity of the solution? Molarity = M b. A…

A: pH = -log[H+] Log [H+] = -pH [H+] = 10-pH

Q: A solution has an OH- concentration of 1.0 x 10-3 mole/L. What is the solution's pH? a. 3.0 b. 4.0…

Q: Which of the solutions listed below has the lowest pH? A. Pure H2O B. 2.5 x 10-5 M HNO3 C.…

A: Lowest pH mean stronger acid and higher pH mean stronger base .

Q: 12. A 8.5 L sample of a 0.28 M HNO3 solution is mixed with 1.6 L of a 0.64 M HC1 solution. What is…

A: A multiple choice question based on pH calculation, which is to be accomplished.

Q: 1. The pH of an aqueous solution that is 2.7 x 10 -3 M HCl is _______. What is the pOH?

A: Note: multiple questions are there but as per bartleby Q &A guidelines I am authorised to answer…

Q: Which of the following chemical species is amphoteric? a. NaOH b. C4H10 c. H2O d. H2SO4 What is…

Q: Determine the molarity of a KOh solution when each of the following amounts of acid neutralizes 25.0…

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

Q: Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2 b. 0.265 M…

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

Q: 3. Calculate the pH of the following aqueous solutions. a. 2.62 x 10-1 M HCl b. 9.6 x 10-12 M HNO3…

A: For a strong acid, the pH can be calculated straightforwardly because, in strong acids, the…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

.A solution is prepared by mixing 2.3 x 104 moles of sodium hydroxide (NaOH) and 4.5 x 10-6 moles of
hydrobromic acid (HBr). Water (H,O) was added until the volume was 1.00 L. What is the pH of this
solution?
a. 9.86
b. 10.21
C. 10.35
d. 11.55

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 by step

Solved in 2 steps with 2 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

44. The pH of a chemical solution is given by the formula pH =-log,[H"] where [H] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). a. What is the pH for a solution for which H* is 0.01? b. What is the pH for a solution for which [H] is 0.001? c. Determine the Hydrogen ion concentration of an orange ( pH = 3.5 )? d. Determine the Hydrogen ion concentration of an orange ( pH = 7.4)?
Which is a conjugate acid base pair in the following equation?H 3PO 4 + H 2O H 3O +1 + H 2PO 4 -1 What is the pH of a solution whose H +1 concentration is 4.0 X 10 -9? a. 4.0 b. 8.4 c. 3.6 d. 9.0 What is the boiling point of a 2.0 m aqueous solution of sodium chloride?(The boiling point elevation constant for water is 0.512 °C/m.) please answer all
A sample of water from a stream has [H3O*]=3.1 × 10-9 M. Which statement below accurately describes this water sample? A. The water sample is acidic. B. The water sample is a basic solution. C. The pOH of the water sample is 8.50. D. pH of the water sample is much les than 7.0. E. The pH of the water sample is 7.5.
An acid mixture contains 0.60 M HClO (Ka = 2.9 × 10−8) and 0.50 M H2O2 (Ka = 2.4 × 10−12). What is the pH of the solution? a. 0.041 b. 0.22 c. 5.96 d. 0.30 e. 3.88
For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. a. 35 mL of 0.15 M H₂SO4 is mixed with 35 mL of 0.30 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. b. 25 mL of 0.45 M formic acid, HCO₂H is mixed with 25 mL of 0.45 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. c. 65 mL of 0.70 M oxalic acid (H₂ C₂O4) is mixed with 130 mL of 0.70 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7.
A 1.0-liter solution contains 0.25 M HF and 0.41 M NaF (Ka for HF is 7.2 x 10-4). What is the pH of this solution? O a. 3.36 O b. 10.64 O c. 2.93 O d. 3.14 O e. 0.21
For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7. a. 85 mL of 0.30 M H2S is mixed with 85 mL of 0.60 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. b. 70. mL of 0.65 M acetic acid, CH3 CO,H is mixed with 70. mL of 0.65 M NaOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7. c. 80. mL of 0.65 M H2SO4 is mixed with 80. mL of 0.65 M NAOH. O The pH of the solution is less than 7. O The pH of the solution is equal to 7. O The pH of the solution is greater than 7.
Calculate the pH of each of these solutions. is the solution acidic, basic, or neutral ?. a. a solution with a OH- concentration of 5.5 x 10-12 M b. a solution with a H3O+ concentration of 3.2 x 10-8 M c. a solution with a pOH of 7.00
A solution of LIOH was found to have a pH of 13.14 at 25 °C. What is the concentration of LIOH? Oa. 2.58 M Оb. 13.14 М Oc. 2.0 x 10-6 M Od. 2.36 M Oe. 0.14 M
One aqueous solution of a strong acid has pH = 1.20, another pH = 1.80. If equal volumes of these two solutions are combined, what is the pH of the resulting solution? O A. 1.10 O B. 1.40 O C. 1.35 O D. 1.55 O E. 1.50
A solution containing only Ba(OH) 2 in water has a pH of 13.9. What is the molar concentration of barium hydroxide in the solution? a. 1.4 M b. 0.70 M c. 0.040 M d. 0.40 M e. 0.020 M
1. Acetic acid is a weak monoprotic acid with Ka = 1.77 x 10¯5. NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. (Assume no volume change occurs.) Calculate the pH of the solution after the addition of 0.0286 mol of NaOH(s). A. 8.502 B. 1.971 C. 12.029 D. 7.000 2.What is the ratio of [A-] / [HA] for a buffer solution of HA with a pH of 7 if the pKa = 5 for HA? A. 100 B. 0.01 C. 10 D. 0.1 3. Titrate 50.0 ml 0.1 M HCN (Ka = 6.2 x 10-10) with 0.10 M NaOH. Calculate the pH at the half-way or midpoint. A. 9.2 B. 7.0 C. 4.8 D. 0.0