Question

Arrange the solutions in order of increasing acidity (from less acidic to more acidic): I. a...

Arrange the solutions in order of increasing acidity (from less acidic to more acidic):

I. a solution with [H3O+] = 4.2 x 10-6 M

II. lemonade, pH = 2.65

III. 0.25 M nitric acid

IV. pickle juice, pH = 3.10

Homework Answers

Answer #1

I. a solution with

II. lemonade,

III. 0.25 M nitric acid

IV. pickle juice,

The order of increasing acidity (from less acidic to more acidic) is

Lower is the pH, higher is the hydrogen ion concentration and higher is the acidity.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. when forming molecular orbitals from atomic orbitals, what is the order of increasing C-H bond...
1. when forming molecular orbitals from atomic orbitals, what is the order of increasing C-H bond strength for the following. I. sp^3 II. sp^2 III. sp a) II<I<III b) III < II < I c) I < II < III d) III < I < II 3. How many different isomers are there for a compound having the molecular formula C3H6O? a) 5 b) 6 c) 7 d) 4 3. What 2 things will change between two resonance structures? a)...
Arrange the following in order of increasing boiling point. Explain how you know. I) CH3CH2OH II)...
Arrange the following in order of increasing boiling point. Explain how you know. I) CH3CH2OH II) CH3CH2CH3 III) H3C-O-CH3 IV) CH3CH2NH2
Calculate the H3O+, OH- and pH of each of the following solutions: i) 1.02g of H2SO4...
Calculate the H3O+, OH- and pH of each of the following solutions: i) 1.02g of H2SO4 diluted to 250ml of solution (assume a diprotic acid) ii) 2.00mL of 0.500 M perchloric acid, HClO4, diluted to 50.0 mL with water (assume that the volumes add!) iii) 4.50 mL of concentrated sodium hydroxide solution (8.5M) diluted to 12.5 L with water iv) 350 mL of an aqueous solution that is 0.20 M in NaCl and 0.15 M in MgCl2. For this question,...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate?...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate? a. HPO42- + H2O = PO43- + H3O+ b. H2PO42- + H2O = H3PO4 + OH- c. H3PO4 + H2O = H2PO4- + H3O+ d. PO43- + H2O = HPO42- + OH- 2. Tina has two aqueous solutions: 1.2 x 10-2 M NaOH and 1.2 x 10-2 M NH3 (KB=1.8x10-5). Which solution has the higher pH? a. the NaOH solution b. the ammonia solution...
A. What is the pH of the following solutions? i. [H3O+] = 1.0 X 10-6 ii....
A. What is the pH of the following solutions? i. [H3O+] = 1.0 X 10-6 ii. [H3O+] = 4.4 X 10-2 B. What volume in mL of 0.115 M sodium hydroxide would neutralize 25.0 mL of a 0.106 M sulfuric acid solution during a titration?
1. What is the pH at the equivalence point for the titration of 50 mL of...
1. What is the pH at the equivalence point for the titration of 50 mL of an aqueous solution of 0.10 M C6H5COOH (benzoic acid) with a 0.2 M NaOH solution at 25°C? (Ka for benzoic acid is 6.28 x 10−5 2. Which of the following sparingly soluble salts would be more soluble in acidic aqueous solutions at 25°C? i. AgCl ii. Mg(OH)2 iii. AgF iv. AuI3
Plasmid isolation 1. Write a set of instructions for preparing Solutions I, II, and III, using...
Plasmid isolation 1. Write a set of instructions for preparing Solutions I, II, and III, using the stock solutions/powders provided below. Solution Volume (mL) Stock solutions/powders available Solution I, the resuspension solution: 15 mM Tris-HCl, pH 8.0, 10 mM EDTA, 100 μg/mL RNase 50 1 M Tris pH 8.0, 0.5 M EDTA 1%(w/v) RNase (boiled for 20 min to remove any DNase activity) Solution II, the alkaline lysis solution: 0.2 N NaOH, 1%(w/v) SDS 25 5 M NaOH 10%(w/v) SDS...
I am having trouble creating a procedure to use to identify five unknown solutions we will...
I am having trouble creating a procedure to use to identify five unknown solutions we will be given in chem lab. The five solutions will be an acid, a base, a chloride salt, a nitrate salt, and a sodium salt. I have to come up with steps to determine which compound is in each category. Only one will be in each solution. Acid- HCl, HNO3, H2SO4 Base - NaOH, NH3, Na2S Chloride Salt - NaCl, BaCl2, CuCl Nitrate Salt -...
Sort the pH of the following mixtures from LOWEST (most acidic) to HIGHEST (most basic): (I)...
Sort the pH of the following mixtures from LOWEST (most acidic) to HIGHEST (most basic): (I) 0.001 mol of HCl added to 1 L water (II) 0.001 mol HCl added to a buffer solution of 0.1 M HCOOH and 0.1 M NaHCOO (pKa=3.75) (III) 0.001 mol HCl added to a buffer solution of 0.1 M NH4Cl and NH3 (pKa=9.25)
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...