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Arada [10]
3 years ago
8

If w/x = 3, what does x/w equal?=

Mathematics
1 answer:
defon3 years ago
5 0

Answer: 6

Step-by-step explanation:

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Which expression could represent the phrase shown? (1 point)
prisoha [69]

Answer:

(6-2)÷3=1

this is the answer

follow me :)))

8 0
2 years ago
Fern knitted 20 scarves over 5 nights. After 8 nights of knitting, how many scarves would fern have made in total.
Studentka2010 [4]

Answer:

Fern will knit 32 scarves in 8 nights.

Step-by-step explanation:

Number of scarves knitted by Fern in 5 night = 20

Relation between number of scarves knitted and number of nights is proportional,

Therefore, Number of scarves knitted (s) ∝ Number of nights spent to knit the scarves (n)

s ∝ n

s = kn

k = \frac{s}{n}

Here, k = proportionality constant

For s = 20 and n = 5,

k = \frac{20}{5}

k = 4 scarves per night

For 8 nights, by using the same proportionality rule,

k = \frac{s}{8}

4 = \frac{s}{8}

s = 32 scarves

Therefore, Fern will knit 32 scarves in 8 nights.

4 0
3 years ago
What are the excluded values v^2 +1 / v^2 -v-6
valentina_108 [34]
The rational expression
\dfrac{v^{2}+1}{v^{2}-v-6}=\dfrac{v^{2}+1}{(v-3)(v+2)}
will be undefined where the denominator is zero. Values of v that make the denominator zero are v=3 and v=-2.

Excluded values of v are -2 and 3.
5 0
3 years ago
Help me with this please<br> who ever is correct gets Brainliest
zimovet [89]

Answer:

ok it is there is no question lol

Step-by-step explanation:

4 0
3 years ago
Read 2 more answers
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}.

7 0
3 years ago
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