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Answer:

334 J/g

Explanation:

The relevant data provided in the question are as follows:

Mass (m) = 1 g

Specific heat of Fusion (Hf) = 334 J/g

Heat (Q) =?

By applying the formula Q = m·Hf, we can calculate the heat released:

Q = m·Hf

Q = 1 x 334

Q = 334 J

Thus, the total heat released amounts to 334 J.

Answer:

The acetic acid concentration is measured at 8.36 M

Explanation:

Step 1: Given data

The volume of acetic acid = 1.00 mL = 0.001 L

The volume of NaOH = 32.40 mL = 0.03240 L

The molarity of NaOH = 0.258 M

Step 2: The balanced reaction equation

CH3COOH + NaOH → CH3COONa + H2O

Step 3: Determining the concentration of acetic acid

b*Ca*Va = a*Cb*Vb

where b = the sodium hydroxide coefficient = 1

where Ca = the acetic acid concentration = TO BE DETERMINED

where Va = the volume of acetic acid = 1.00 mL = 0.001L

where a = the acetic acid coefficient = 1

where Cb = the sodium hydroxide molarity = 0.258 M

where Vb = the volume of NaOH = 32.40 mL = 0.03240 L

Ca * 0.001 L = 0.258 * 0.03240

Ca = 8.36 M

The acetic acid concentration is 8.36 M

Response:

1) The bubbles will expand, and additional ones might surface.

2) Can A will produce a more intense and resonant fizz than Can B.

Explanation:

By compressing the bottle's sides, the pressure exerted increases on the bubbles, forcing them into a smaller area. This reduction in volume results in an increased density of the bubble. When density rises, the bubble enlarges and new bubbles can form. Consequently, altering the pressure (by squeezing the bottle) modifies the bubble sizes while retaining the number of bubbles. In carbonated beverages, higher temperatures cause a quicker loss of fizz due to the increased volatility of carbon dioxide in liquids at elevated temperatures. This principle explains that carbon dioxide's solubility in can A at 32°C is lower than in can B at 8°C, making can A's fizz louder compared to can B's.

Answer:

D) NaO2CC6H4CO2K

Explanation:

Water acts as a polar solvent and is known to solvate polar substances. This characteristic allows solute molecules to engage with the solvent, resulting in increased solubility of a molecule as its polarity rises. Consequently, the salt derived from phthalic acid shows greater solubility in water compared to phthalic acid itself. Although both monosodium and monopotassium salts exhibit higher solubility than phthalic acid, the dialkali phthalate salt (NaO2CC6H4CO2K) possesses the highest solubility due to its greater polarity.