### Arranging Solutions by pH**Assuming equal concentrations, arrange these solutions by pH, from highest to lowest.**#### Solutions List- **HCN(aq)**- **HI(aq)**- **NH₃(aq)**- **Sr(OH)₂(aq)**- **RbOH(aq)**For a better understanding of how to arrange these solutions by pH, consider the following points:1. **RbOH (Rubidium Hydroxide)**: A strong base which should have the highest pH.2. **Sr(OH)₂ (Strontium Hydroxide)**: Another strong base, which also results in a high pH, but slightly lower than RbOH because alkali metal hydroxides are generally stronger.3. **NH₃ (Ammonia)**: A weak base, resulting in a moderately high pH.4. **HCN (Hydrogen Cyanide)**: A weak acid, resulting in a slightly acidic pH.5. **HI (Hydroiodic Acid)**: A strong acid, which should have the lowest pH.### Answer BankThe rank from highest to lowest pH will look like this:1. **RbOH(aq)**2. **Sr(OH)₂(aq)**3. **NH₃(aq)**4. **HCN(aq)**5. **HI(aq)**

Answered: Image /qna-images/answer/6ffd109b-bf45-4a5c-98c1-cc45f28d05fe.jpg

Answered: of 45 > Assuming equal concentrations,…

of 45 > Assuming equal concentrations, arrange these solutions by pH. Highest pH HCN(aq) HI(aq) NH,(aq) Sr(OH)₂ (aq) RbOH(aq) Lowest pH Answer Bank

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: Starting with 0.1 mol L−1 HNO2(aq), which one of the following operations would cause the pH of the…

Q: A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar…

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

Q: A solution is prepared that is initially 0.22M in nitrous acid (HNO,) and 0.49M in potassium nitrite…

Q: For the titration of 20.0 mL of 0.400 M HCl(aq) with 0.400 M NaOH(aq): 1. What is the initial pH of…

A: we have to calculate the pH of solution

Q: Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution…

A: we need to calculate the change in pH for the given solutions

Q: A 0.263 g sample of Na2CO3 requires 28.35 mL of HCl to completely react with it. What is the pH of…

Q: Which statement is true concerning the buffer system below? HA(aq) + H2O0 2 H;O* (aq) + A (ba) (be)…

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

Q: An analytical chemist is titrating 200.5 mL of a 0.3400M solution of hydrazoic acid (HN,) with a…

A: Here we use the Henderson Hasselbach equation,pH = pKa + log [Salt]/[Acid] Initial Acid = 200.5 x…

Q: Consider a buffer solution that consists of two separate components: the weak acid ch3coo aq), and…

A: In the given question, buffer of weak acid and its conjugate base is given i.e., CH3COOH and…

Q: A solution is prepared that is initially 0.12M in hydrofluoric acid (HF) and 0.061 M in sodium…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: An analytical chemist is titrating 113.4 mL of a 0.7600M solution of 4.74. Calculate the pH of the…

Q: 22) Consider the titration of a 50.00 mL sample of 0.200 M benzoic acid with 0.200 M NaOH (aq., 25…

A: Given, Molarity of benzoic acid (C6H5COOH) = 0.200 M Volume of C6H5COOH = 50.00 mL Molarity of…

Q: One function of our blood is to carry CO2CO2 from our tissues to our lungs. It is critical that the…

Q: Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all…

A: It refers to the acid dissociation constant having the significance of that fact that how much or…

Q: A solution is prepared that is initially 0.34M in acetic acid (HCH,CO, and 0.33M in potassium…

A: Molarity of acetic acid = 0.34 MMass of potassium acetate =0.33 M

Q: A chemist titrates 230.0 mL of a 0.1110 M pyridine (C5H;N) solution with 0.7963 M HNO, solution at…

Q: Consider a buffer solution at 25°C that consists of 0.29 M HOCl(aq) and 0.23 M NaOCl(aq).…

A: The objective of this question is to calculate the pH of a buffer solution. The buffer solution is…

Q: What is the equilibrium constant expression for the following reaction ? PbF2(s)=Pb2+(aq)+2F-(aq)

A: Given equilibrium is PbF2(s) <---> Pb2+(aq) + 2F-(aq) We need to write an expression for its…

Q: The reaction of the weak acid HCN with the strong base KOH is HCN(aq) + KOH(aq) HOH(1) + KCN(aq) To…

Q: A chemist titrates 130.0 mL of a 0.8034M pyridine (C,HşN) solution with 0.2958M HCl solution at 25…

Q: Calculate the pH of the resulting solution if 25.0 mL of 0.250 M HCI(aq) is added to 30.0 mL of…

Q: Calculate the pH for a solution that contains 3.0*10-3M CsOH (aq)

A: The objective of this question is to calculate the pH of a solution containing 3.0*10^-3 M CsOH…

Q: need help with the explanation under the table.

A: Le Chatlier Principle states that if a system at dynamic equilibrium is disturbed by change in…

Q: A chemist titrates 60.0 mL of a 0.4543 M aniline (C,H;NH,) solution with 0.7673M HNO, solution at 25…

Q: Calculate the change in pH when 9.00 of 0.100 M HCl * (aq) is added to 100.0 of a buffer solution…

Q: The pKp values for the dibasic base B are pKbl = 2.10 and pKb2 = 7.65. Calculate the pH at each of…

A: pH is a scale which basically measure the acidity/ basicity of a solution. If PH value is 7 then…

Q: Using only the Henderson-Hasselbalch equation, what is the pH of a solution that is 0.22M phenol,…

A: Given: Molarity of phenol = 0.22 M Molarity of sodium phenoxide = 0.29 M Ka of phenol = 1.3×10-8

Q: Which choice below will increase the pH of a 0.2 M H2S solution? Group of answer choices Bubble…

A: H2S <---> 2H+ + S2- Anything which will lead to decrease in the concentration of H+ will…

Q: OHI(aq) + NH4OH(aq) = H₂O(l) + NH4l(aq) O H3O+ (aq) + NH4OH(aq) = H₂O(l) + NH4+ (aq) O HI(aq) +…

A: •STRONG ACID:- Acid which dissociate completely in solution are called strong acid. :-EXAMPLE:- HI,…

Q: 2.500 g of an unknown achiral primary amine is dissolved in enough water to yield a 50.00 mL…

A: Given : mass of primary amine used = 2.500 g concentration of HCl used = 0.9250 M And volume of HCl…

Q: The pK, values for the dibasic base B are pKbl = 2.10 and pKb2 = 7.38. Calculate the pH at each of…

A: pkb1 = 2.10 pkb2 = 7.38 [B] = 0.95 M [HCl] = 0.95 M V = 50.0 mL

Q: Cl2(aq) reacts with H,O(€) as follows: Cl2 (aq) + 2 H20(€) 2H;0* (aq) + Cl¯(aq) + HOCI(aq) For an…

A: In order to find the answer to the above question we try to analyze the given data: The reactants of…

Q: Propionic acid, HC3H5O2, has a Ką value of 1.3 x 105. A buffer solution is prepared by mixing 20.0…

A: Given:- Propionic acid, HC3H502, has a Ką value of 1.3 x 10-5. A buffer solution is prepared by…

Q: What will happen if the pH of the following equilibrium system is increased? H*(aq) + 2CrO4²a 2- aq)…

A: So option a is correct that is the solution will turn yellow

Q: A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K,HPO4. Determine the pH change when 0.061…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: Which of the following solutions will h

A: the solutions which resists change in pH by the addition of small amount of strong acid (or) base…

Q: 9 rea Use the References to access important values if needed for this question. A buffer solution…

A: Given Concentration of NaH2PO4 = 0.474 M Concentration of K2HPO4 = 0.290 M Volume = 125 ml = 125 x…

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

### Arranging Solutions by pH

**Assuming equal concentrations, arrange these solutions by pH, from highest to lowest.**

#### Solutions List
- **HCN(aq)**
- **HI(aq)**
- **NH₃(aq)**
- **Sr(OH)₂(aq)**
- **RbOH(aq)**

For a better understanding of how to arrange these solutions by pH, consider the following points:

1. **RbOH (Rubidium Hydroxide)**: A strong base which should have the highest pH.
2. **Sr(OH)₂ (Strontium Hydroxide)**: Another strong base, which also results in a high pH, but slightly lower than RbOH because alkali metal hydroxides are generally stronger.
3. **NH₃ (Ammonia)**: A weak base, resulting in a moderately high pH.
4. **HCN (Hydrogen Cyanide)**: A weak acid, resulting in a slightly acidic pH.
5. **HI (Hydroiodic Acid)**: A strong acid, which should have the lowest pH.

### Answer Bank
The rank from highest to lowest pH will look like this:

1. **RbOH(aq)**
2. **Sr(OH)₂(aq)**
3. **NH₃(aq)**
4. **HCN(aq)**
5. **HI(aq)**

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

If the pH of a 0.200 M solution of the CICH2O¯ ion is 12.05, then what is the value for the basicity constant, Kp, of CICH20-? You do not need to make a simplifying assumption CICH,0-(aq) + H2O(1) СICH-OОH(aq) + ОН (аq) K½ = ?
CH3CH₂COOH(aq) + H₂O(l) + ← CH3CH₂COO (aq) + H30* (aq) Propanoic acid, CH3CH₂COOH, is a carboxylic acid that reacts with water according to the equation above. At 25°C the pH of a 34.0 mL sample of 0.22 M CH3CH2COOH is 2.75. Determine the value of Ka for propanoic acid at 25°C (do not look up the answer on the internet, because some of the numbers have been changed in the problem). (Write your answer in scientific notation) Ka= Submit Question 349 45,838 ty MAY 23 @
Using the equation below, explain what happens to maintain the pH of the solution: HA (aq)= H+ (aq)+A- (aq) (i) when an acid is added (ii) when a base is added
Formic acid, HCOOH, is the simplest of the carboxylic acids and occurs naturally, most notably in some ants. If the formate (HCOO–) concentration is 0.100 M, determine the formic acid (HCOOH) concentration required to buffer a solution at pH = 3.35 HCOOH(aq) ↔ HCOO–(aq) + H+(aq) Ka = 1.80 × 10-4 i) Calculate the pKa of the acid and provide your final answer with 3 decimal places ii) Write the main equation that you will use to help you calculate the formic acid concentration iii) Calculate the formic acid concentration required to buffer the solution at pH = 3.35 and provide your final answer with 3 decimal places
Calculate the pH of a solution prepared by dissolving 0.482 mol of benzoic acid and 0.104 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K, of benzoic acid is 6.30 x 105. CHSCOOH(aq) + H2O(1) = H3O*(aq) + C6H5CO2 (aq) K = 6.30 × 10-5 A pH = pK, + log; [HA] [* ] %3D
Which statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium acetate (NaCH3COO)? How does a buffer resist change in pH upon addition of a strong acid? By titration, it is found that 73.3 mL of 0.189 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
Calculate the change in pH when 5.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq)NH3(aq) and 0.100 M in NH4Cl(aq).NH4Cl(aq). Consult the table of ionization constants as needed. Link for table of ionization constants: Chempendix - Ionization Constants (google.com) Calculate the change in pH when 5.00 mL of 0.100 M NaOH is added to the original buffer solution.
7
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M H3O+ M OH-
An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M solution of HIO,. The p K, of ammonia is 4.74. Calculate 3' the pH of the base solution after the chemist has added 99.0 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places.
A chemist titrates 100.0 mL of a 0.0714M nitrous acid (HNO,) solution with 0.3683M KOH solution at 25 °C. Calculate the pH at equivalence. The p K, of nitrous acid is 3.35. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = |
Is it possible if u can get back to me asap when u see this??!~