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Answer the following statements by writing True or False? Statement The pOH of a 0.0010 M HCl is 3 Strong acid \( [H^+] = [HCl] \) \(pOH = 14 - pH \) \(pH = -Log(0.001) = 3 \) \(14 - 3 = 11\) \(pH + pOH = -pKw\) The pH of 1.0 x 10<sup>-9</sup> M HCl is 9.0 If water produces 10<sup>-8</sup> M OH it must produce 10<sup>-6</sup> M H<sup>+</sup>. For weak bases equilibriums, K<sub>b</sub> is called base hydrolysis constant The fraction of dissociation (\(\alpha\)) of weak acids is proportional inversely with acid concentration. Na<sub>2</sub>CO<sub>3</sub>/NaHCO<sub>3</sub> can be used as a buffer system because CO<sub>3</sub><sup>2-</sup> is a weak base and HCO<sub>3</sub><sup>-</sup> is its conjugate acid. Buffers usually have a usable range within ±1 pH unit of pKa (i.e, a range of pH = pKa ± 1).

          Answer the following statements by writing True or False?
Statement
The pOH of a 0.0010 M HCl is 3 Strong acid \( [H^+] = [HCl] \)
\(pOH = 14 - pH \) \(pH = -Log(0.001) = 3 \) \(14 - 3 = 11\)
\(pH + pOH = -pKw\)
The pH of 1.0 x 10<sup>-9</sup> M HCl is 9.0
If water produces 10<sup>-8</sup> M OH it must produce 10<sup>-6</sup> M H<sup>+</sup>.
For weak bases equilibriums, K<sub>b</sub> is called base hydrolysis constant
The fraction of dissociation (\(\alpha\)) of weak acids is proportional inversely
with acid concentration.
Na<sub>2</sub>CO<sub>3</sub>/NaHCO<sub>3</sub> can be used as a buffer system because CO<sub>3</sub><sup>2-</sup> is a
weak base and HCO<sub>3</sub><sup>-</sup> is its conjugate acid.
Buffers usually have a usable range within ±1 pH unit of pKa (i.e, a range
of pH = pKa ± 1).

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$Answer the following statements by writing True or False? Statement The pOH of a 0.0010 M HCl is 3 Strong acid [H^+] = [HCl] pOH = 14 - pH pH = -Log(0.001) = 3 14 - 3 = 11 pH + pOH = -pKw The pH of 1.0 x 10<sup>-9</sup> M HCl is 9.0 If water produces 10<sup>-8</sup> M OH it must produce 10<sup>-6</sup> M H<sup>+</sup>. For weak bases equilibriums, K<sub>b</sub> is called base hydrolysis constant The fraction of dissociation (α) of weak acids is proportional inversely with acid concentration. Na<sub>2</sub>CO<sub>3</sub>/NaHCO<sub>3</sub> can be used as a buffer system because CO<sub>3</sub><sup>2-</sup> is a weak base and HCO<sub>3</sub><sup>-</sup> is its conjugate acid. Buffers usually have a usable range within ±1 pH unit of pKa (i.e, a range of pH = pKa ± 1).$

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert David Collins

10/23/2020

Step 1

Since HCl is a strong acid and completely dissociates in water, the concentration of OH- in a 0.0010 M HCl solution is negligible. Therefore, the pOH of the solution is 0. Step 2: The equation pH + pOH = 14 is used to relate the pH and pOH of a solution. Since Show more…

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Texts: are these answers correct? Answer the following statements by writing True or False. Statement True or False The pOH of a 0.0010 M HCl is 3. True [H+] = HCl pH + pOH = -pKw True The pH of 1.0x10^-9 M HCl is 9.0. False If water produces 10^-14 M OH-, it must produce 10^-14 M H+. True For weak bases, the equilibrium constant K is called the base hydrolysis constant. True The fraction of dissociation (a) of weak acids is inversely proportional to acid concentration. False NaCO/NaHCO can be used as a buffer system because CO3^2- is a weak base and HCO3^- is its conjugate acid. Buffers usually have a usable range within 1 pH unit of pKa (i.e., a range of pH = pKa ± 1). False

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00:01 Question number 64 is a very good review of this chapter by having you answer a series of true and faults, or having you determine whether or not a series of statements are true or false.

00:19 The first statement that is provided is all bronzed lowry acids are arrainious acids.

00:27 Now normally we think that the bronze sted lowry definition is much broader.

00:32 Than the arraneous definition, and it is, and that extended broadness really comes into play with bases more so than with acids.

00:42 So we can state that all bronstead -lowry acids are arraneous acids, and all arraneous acids are bronsted -lowry acids.

00:52 However, in the case of bases, this is not always true.

00:56 We can't state that all arranius bases are bronstead lowry bases.

01:02 I'm sorry, we can state that all arranius bases are bronsted lowry bases, but we cannot state that all bronsstead lowry bases are arraneous bases, the bronstead -lowry definition being more broad, so there's likely to be some bronsted -lowry bases that do not fall under the umbrella of the arraneous definition.

01:25 So this statement is true.

01:29 Part c gives us bicarbonate and states that it is amphoteric or that it can behave as an amphoteric species.

01:39 This is true.

01:41 It's negatively charged so it could take on another hydrogen ion and become carbonic acid, or it could give up its hydrogen ion.

01:48 If it gives it up, it's acting as an acid.

01:51 If it accepts one, it's acting as a base, and that's the definition of amphoteric, being able to act as an acid or a base.

01:59 Part d gives us hs minus and states that it is the conjugate base to s2 minus.

02:07 It is a conjugate to s2 minus, but it's actually the conjugate acid of s2 minus, not the conjugate base.

02:15 So this is false.

02:18 Part e then says that if there is more product, then the equilibrium is going to favor the forward direction.

02:30 This is true.

02:31 Anytime we get more product at equilibrium, the equilibrium favors the forward direction.

02:38 If we have less product or we have more reactant, then the equilibrium favors the reverse direction.

02:46 Part f gives us nh4 plus and says it cannot act as a lewis base.

02:53 To act as a lewis base, it must have an electron pair to donate.

02:57 You draw the lewis structure of n4h, or sorry, nh4.

03:02 4 plus and it doesn't have a loan pair anywhere...

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