Hydroiodic Acid And Potassium Hydroxide

TheAbsoluTurk

Homework Statement

Rest the following equation and write the corresponding
ionic and cyberspace ionic equation (if appropriate):

CH[itex]_{3}[/itex]COOH [itex]_{(aq)}[/itex]+ KOH [itex]_{(aq)}[/itex] [itex]\rightarrow[/itex]

Homework Equations

None as far every bit I know.

The Attempt at a Solution

I wrote:

CH[itex]_{3}[/itex]COOH [itex]_{(aq)}[/itex]+ KOH [itex]_{(aq)}[/itex] [itex]\rightarrow[/itex] CH[itex]_{3}[/itex]Cook [itex]_{(aq)}[/itex] + H[itex]_{2}[/itex]O [itex]_{(l)}[/itex]

Only this is the incorrect respond.

I don't sympathize why Grand[itex]^{+}[/itex] does not form a compound with CH[itex]_{iii}[/itex]COO[itex]^{-}[/itex]. Tin anyone tell what concept or law/theorem controls what compounds form and what compounds practice not form? Why is K[itex]^{+}[/itex] a spectator ion in this reaction?

Borek

Your reaction equation is OK, information technology just doesn't answer the question - you were asked to write ionic and net ionic reactions. Which of the compounds present in the reaction will be fully dissociated?

Notation: format indices in your formulae with [noparse] and [/noparse] tags, not with LaTeX. And state of affair should be normal text, on the aforementioned level as the formula (so dissolved potassium acetate is [noparse]CH₃Cook(aq)[/noparse] - rendered equally CH₃Melt(aq)).

TheAbsoluTurk · May 14, 2013

Your reaction equation is OK, it just doesn't answer the question - you were asked to write ionic and net ionic reactions. Which of the compounds present in the reaction volition be fully dissociated?
Notation: format indices in your formulae with [noparse] and [/noparse] tags, not with LaTeX. And state of matter should exist normal text, on the aforementioned level as the formula (so dissolved potassium acetate is [noparse]CH₃COOK(aq)[/noparse] - rendered every bit CH_threeCook(aq)).

And so my initial line of thinking was:

Molecular Equation:
CH₃COOH (aq)+ KOH (aq) → CH₃Cook (aq) + H₂O (50)

Ionic Equation:

CH₃COO^- (aq) + H⁺ (aq) + K⁺ (aq) + OH^- (aq) → CH_threeCOO^- + Thousand⁺ + H₂O (l)

Internet Ionic Equation:

H⁺ (aq) + OH^- (aq) → H₂O (fifty)

This is incorrect.

Simply I reasoned that CH_threeCOO^- is a weak acid and so all of the things in the textbook about not dissociating 100% must come into play hither.

Therefore,

Molecular Equation:
CH_iiiCOOH (aq)+ KOH (aq) → CH₃COOK (aq) + H_iiO (l)

Ionic Equation:

CH₃COOH (aq) + K⁺ (aq) + OH^- (aq) → CH_threeCOO^- +K⁺ + H_iiO (l)

Net Ionic Equation:

CH₃COOH (aq) + OH^- (aq) → CH₃COO^- + H_iiO (fifty)

That is right according to the answers in the text.

How come up CH_iiiCOO^- and 1000⁺ do not class a compound though? Is there anyway to summate or know why? Is it because CH₃COOH is non dissociated 100% in solution? (information technology is a weak acid.)

Cheers for the help with writing the equations.

TheAbsoluTurk

In the ionic equation, Thousand+ and CH3COO- are dissociated because CH3COOK is a strong electrolyte. While CH3COOK is a weak acid and so information technology doesn't dissociate 100%.

Is this correct. I'grand surprised the text doesn't explain this. Borek, can you recommend any comprehensive, first year academy chemistry textbooks?

Borek

How come CH₃COO^- and K⁺ do not form a compound though?

Imagine a solution containing equal concentrations of CH_iiiCOO^-, Cl^-, K⁺ and Na⁺ - y'all tin can't tell what compounds it contains, at that place is more than 1 answer. Then we don't name these compounds at all, it is safer to simply listing ions.

Sorry, I can't be of much help when it comes to books - unless y'all are interested in Polish ones Chang and Pauling are normally praised as good titles.

TheAbsoluTurk

Imagine a solution containing equal concentrations of CH₃COO^-, Cl^-, K⁺ and Na⁺ - you can't tell what compounds it contains, there is more one respond. So nosotros don't proper name these compounds at all, it is safer to simply list ions.
Pitiful, I can't be of much assistance when it comes to books - unless y'all are interested in Polish ones Chang and Pauling are usually praised equally good titles.

And then the explanation that "In the ionic equation, K+ and CH3COO- are dissociated because CH3COOK is a strong electrolyte. While CH3COOH is a weak acid so it doesn't dissociate 100%." is incorrect? Or it doesn't make sense?

I'g reading Chang correct now actually.

TheAbsoluTurk

In the ionic equation, Yard+ and CH3COO- are dissociated because CH3COOK is a stiff electrolyte. While CH3COOK is a weak acid then it doesn't dissociate 100%.

Is this correct. I'm surprised the text doesn't explain this. Borek, tin can you recommend any comprehensive, first yr university chemistry textbooks?

I meant to say CH3COOH is a weak acrid, non CH3COOK. My idea is that CH3COOK is a stiff electrolyte so it dissociates 100% in solution therefore leaving K+ and CH3COO- in solution.

Borek

I meant to say CH3COOH is a weak acid, not CH3COOK. My idea is that CH3COOK is a strong electrolyte and then it dissociates 100% in solution therefore leaving Yard+ and CH3COO- in solution.

This role was OK, I only tried to reply your other question.

TheAbsoluTurk

This part was OK, I just tried to respond your other question.

Oh, ok. I idea the two questions answered the same thing. Anyway I accept a meliorate thought of how to tell what products will arise from certain reactants. Thanks for the help.

Hydroiodic Acid And Potassium Hydroxide

Reaction of acetic acid (CH3COOH) with potassium hydroxide (KOH)

Homework Statement

Homework Equations

The Attempt at a Solution

Answers and Replies

Suggested for: Reaction of acetic acid (CH3COOH) with potassium hydroxide (KOH)

Hydroiodic Acid And Potassium Hydroxide,

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