Of the following, which are characteristics of basic solutions? (Select all that apply)
Select all that apply:
pH levels less than 7 at 25°C
Greater concentration of hydroxide ions than hydronium ions
[H3O+]< [OH-]
pH levels of 7 at 25°C
Basic solutions have
1) pH level more than 7
2) Concentration of hydroxide ions is more than that of hydronium ions.
So options b and c are correct
Calculate the pH and pOH of the solutions with the following hydronium ion [H3O+] or hydroxide ion [OH–] concentrations. Determine which solutions are acidic, basic or neutral. (1.a) [OH–] = 8.2 × 10–11 M (1.b) [OH–] = 7.7 × 10–6 M (1.c) [H3O+] = 3.2 × 10–4 M (1.d) [H3O+] = 1.0 × 10–7 M
The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, pH=−log[H3O+] In neutral solutions at 25 ∘C, [H3O+]=10−7 M and pH=7. As [H3O+] increases, pH decreases, so acidic solutions have a pH of less than 7. Basic solutions have a pH greater than 7. Calculate the pH of a 0.10 M solution of HCl. Express your answer numerically using two decimal places.
3) Indicate the concentration of hydrogen ions or hydroxide ions in the following solutions. When appropriate, use greater than or less than symbols. a) 0.15 M HNO3 c) 0.75 M KOH b) 1.0 M H2SO4 (whether it is 1M, 2M, or between 1M and 2M) d) 0.10 M Ba(OH)2 4) Give the hydronium and hydroxide ion concentrations for the following solutions: a) 2.25 x 10' M NaOH c) 0.0115 M Ca(OH)2 b) 0.25 M HNO3
Which of the following statements describes a basic solution? 1. [H30+]> [OH] 2. [H30]<[OH] 3. [H30'] x [OH] #1 x 10-14 4. [H3O+]/[OH] = 1 x 10-14 5. [H3O+]/[OH]=1 If the pH of a solution is 10, what is the hydronium, H ion concentration? 1. A) 1 x 10-10 M 2. B) 1 x 1010 M 3. C) 10 M 4. D) 10 M 5.E) * 1 1010 M As the pH increases the hydroxide ion concentration 1. A) goes...
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Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? In acids, [OH-] is less than [ H30+). In acids, [OH-] = [H3O+]. In neutral solutions, [H3O+] = [H20). In bases, [H3O+] is more than [H20] In acids, [OH-] is greater than [H3O+]. O
Typically the concentration of hydronium, H3O+, or hydroxide, OH−, ions in an aqueous solution is less than 1 M. It is not uncommon to have hydronium ion concentrations that are much smaller, such as 2.60×10−5. pH, therefore, is a convenient way to restate the hydronium concentration. pH is equal to the negative log of a hydronium ion concentration in solution: pH=−log[H3O+] Access the pH calculation simulation, which will open in a new window. Edit the concentration by typing a value...
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Revised 02/19/2009 Mill- Practice Quiz for Chapter 16 (Note, you should not necessarily expect multiple choice questions on the test.) Hydride ion H' is a stronger base than hydroxide ion OH. Complete the following reaction > H' (aq) + H2O (l) What is the molar concentration of hydronium ion H,O in pure water at 25° C? What is the molar concentration of hydroxide ion OH if the solution pH is 4.282 at 25 C? Calculate the molar concentration of...
1) Which of the following best indicates the meaning of the term autoionization? Select the correct answer below: a)Autoionization is a reaction involving the transfer of a proton from an acid to water, yielding hydronium ions and the conjugate base of the acid. b)Autoionization is a reaction involving the transfer of a proton from water to a base, yielding hydroxide ions and the conjugate acid of the base. c)Autoionization is a reaction between two molecules of the same neutral substance...
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Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
Complete the following table. (All solutions are at 25 ?C.) [H3O+] [OH?] pH Acidic or Basic _____ _____ 3.15 _____ 3.7