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NeTakaya
3 years ago
9

In ΔABC, m∠ACB = 90°, CD ⊥ AB and m∠ACD = 45°. Find: CD, if BC = 3 in

Mathematics
2 answers:
IRISSAK [1]3 years ago
4 0
We can find m∠BCD like follows: m∠BCD=90°-45°=45<span>°
Now, m</span><span>∠DBC= 180°-(90°+45°)=45°

Remember that </span>sin \alpha = \frac{opposite leg}{hypotenuse}, so oppositeleg=(hypotenuse)(sin \alpha )

We know that hypotenuse= BC= 3in and \alpha=∠DBC)=45°, so replacing the values we get:
CD=3sin(45)=2.12

We can conclude that the segment CD is 2.12 in
finlep [7]3 years ago
4 0

Given ΔABC,

m∠ACB = 90 degrees,

CD ⊥ AB

m∠ACD = 45 degrees

BC = 3 in

CD is unknown

 

To know the Length of CD, we use the trigonometric function Cos Ɵ = A/H

If ∠BCD is Ɵ,

H = BC = 3 in

A = CD (Unknown)

 

m∠ACD + m∠BCD = m∠ACB

m∠BCD = m∠ACB – m∠ACD

m∠BCD = 90 degrees – 45 degrees

m∠BCD = 45 degrees

Therefore, Ɵ = m∠BCD = 45 degrees

 

Cos Ɵ = A/H

Cos 45 = CD/3

CD = 3 Cos 45

CD= 3 x 0.7071

CD = 2.1213

CD is approximately 2.12 in

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Answer:

60

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Calculate the pH of a buffer solution made by mixing 300 mL of 0.2 M acetic acid, CH3COOH, and 200 mL of 0.3 M of its salt sodiu
Lesechka [4]

Answer:

Approximately 4.75.

Step-by-step explanation:

Remark: this approach make use of the fact that in the original solution, the concentration of  \rm CH_3COOH and \rm CH_3COO^{-} are equal.

{\rm CH_3COOH} \rightleftharpoons {\rm CH_3COO^{-}} + {\rm H^{+}}

Since \rm CH_3COONa is a salt soluble in water. Once in water, it would readily ionize to give \rm CH_3COO^{-} and \rm Na^{+} ions.

Assume that the \rm CH_3COOH and \rm CH_3COO^{-} ions in this solution did not disintegrate at all. The solution would contain:

0.3\; \rm L \times 0.2\; \rm mol \cdot L^{-1} = 0.06\; \rm mol of \rm CH_3COOH, and

0.06\; \rm mol of \rm CH_3COO^{-} from 0.2\; \rm L \times 0.3\; \rm mol \cdot L^{-1} = 0.06\; \rm mol of \rm CH_3COONa.

Accordingly, the concentration of \rm CH_3COOH and \rm CH_3COO^{-} would be:

\begin{aligned} & c({\rm CH_3COOH}) \\ &= \frac{n({\rm CH_3COOH})}{V} \\ &= \frac{0.06\; \rm mol}{0.5\; \rm L} = 0.12\; \rm mol \cdot L^{-1} \end{aligned}.

\begin{aligned} & c({\rm CH_3COO^{-}}) \\ &= \frac{n({\rm CH_3COO^{-}})}{V} \\ &= \frac{0.06\; \rm mol}{0.5\; \rm L} = 0.12\; \rm mol \cdot L^{-1} \end{aligned}.

In other words, in this buffer solution, the initial concentration of the weak acid \rm CH_3COOH is the same as that of its conjugate base, \rm CH_3COO^{-}.

Hence, once in equilibrium, the \rm pH of this buffer solution would be the same as the {\rm pK}_{a} of \rm CH_3COOH.

Calculate the {\rm pK}_{a} of \rm CH_3COOH from its {\rm K}_{a}:

\begin{aligned} & {\rm pH}(\text{solution}) \\ &= {\rm pK}_{a} \\ &= -\log_{10}({\rm K}_{a}) \\ &= -\log_{10} (1.76 \times 10^{-5}) \\ &\approx 4.75\end{aligned}.

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Answer:

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