A11.8-gram sample of zinc is heated to 98.15°c in a boiling water bath. the hot metal is then immersed in 25.35 grams of water that is initially at 21.82°c. at what temperature will the metal and the water reach thermal equilibrium? the specific heat of zinc is 0.388 j/g·°c. the specific heat of water is 4.184 j/g·°c.

T =24.98 °C

Explanation:

from equilibrium condition we have:

[m_1*s*T]_{water} = [m_2*s*T]_{zinc}

Where

m_1 , m_2 is mass of water and zinc respectively

s denote specific heat

let final equilibrium temperature is T

25.35*4.184*[T-21.82] = 11.8*0.388*[98.15-T]

106.06T - 2314.32 = 449.36 - 4.57T

110.63 T =  2763.68

T =24.98 °C

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i have found an answer to your question but use it as information.

information: because weak acids/bases have low concentration of hydrogen ions, the addition of water has a large impact on the ph. 2. a difference in 1 unit is a 10x difference in concentration for example; a liquid with ph of 3 is 10x more acidic than a liquid with a ph of 4. therefore, a liquid with a ph of 3 is stronger.

best of luck!

unbalanced force

explanation: