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elena55 [62]
1 year ago
10

Explain with equations and calculations, when necessary, whether an aqueous solution of each of these salts is acidic, basic, or

neutral:(CH₃)₂NH₂ Br
Chemistry
1 answer:
Lelechka [254]1 year ago
4 0

(CH₃)₂NH₂Br is an acidic salt.

<h3>What are acidic salts?</h3>

Neutralization of a strong acid with a weak base gives an acidic salt.

Examples: Ammonium chloride, Copper sulfate, Silver nitrate

<h3>What are basic salts?</h3>

Neutralization of a weak acid with a strong base gives a basic salt.

Examples: Sodium Acetate, Potassium cyanide, Sodium sulfide

<h3>What are neutral salts?</h3>

They are formed by the neutralization of strong acids and strong bases, are called neutral salts because their aqueous solutions are neutral to litmus.  

Examples: The compounds like NaCl, KCl, K2S04, NaN03, KCl03, KClO4 etc. are neutral salts.

To learn more about salts: brainly.com/question/5306491

#SPJ4

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What is the freezing point of an aqueous solution that has 25.00 g of calcium iodide dissolved in 1250 g of water?
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Answer:

<u></u>

  • <u>- 0.380ºC</u>

Explanation:

The lowering of the freezing point of a solvent is a colligative property ruled by the formula:

  • \Delta T_f=K_f\times m\times i

Where:

  • ΔTf is the lowering of the freezing point
  • Kf is the molal freezing constant of the solvent: 1.86 °C/m
  • m is the molality of the solution
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<u />

<u>a) molality, m</u>

  • m = number of moles of solute/ kg of solvent
  • number of moles of CaI₂ = mass in grams/ molar mass
  • number of moles of CaI₂ = 25.00g / 293.887 g/mol = 0.0850667mol
  • m = 0.0850667mol/1.25 kg = 0.068053m

<u>b) i</u>

  • Each unit of CaI₂, ideally, dissociates into 1 Ca⁺ ion and 2 I⁻ ions. Thus, i = 1 + 2 = 3

<u />

<u>c) Freezing point lowering</u>

  • ΔTf =  1.86 °C/m × 0.068053m × 3 = 0.3797ºC ≈ 0.380ºC

<h2>I have problems to upload the full answer in here, so I attach a pdf file with the whole answer.</h2>
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