This is a neutralisation reaction, so we know that the products formed are salt and water.
First, we balance the chemical equation:
KOH + HNO3 ----> KNO3 + H2O.
After that, we split the compounds into their respective charges.
K+ + OH- + H+ + NO3- ----------> K+ + NO3- + H2O*
(*note that liquid cannpt be splitted.)
After that we reduce the chemical equation by removing the common ones.
OH- + H+ --------> H2O
Tada.
Answer:
<h2>pOH = 9.52</h2>
Explanation:
The pOH of the solution can be found by using the formula
pH + pOH = 14
Since we are finding pOH we have
pOH = 14 - pH
From the question
pH = 4.48
Substitute the value into the above formula and solve for the pOH
That's
pOH = 14 - 4.48
We have the final answer as
<h3>pOH = 9.52</h3>
Hope this helps you
The number of electrons that goes into a Lewis Model is determined by the number of valence electrons
Answer : The partial pressure of
and
is, 216.5 mmHg and 649.5 mmHg
Explanation :
According to the Dalton's Law, the partial pressure exerted by component 'i' in a gas mixture is equal to the product of the mole fraction of the component and the total pressure.
Formula used :
![p_i=X_i\times p_T](https://tex.z-dn.net/?f=p_i%3DX_i%5Ctimes%20p_T)
![X_i=\frac{n_i}{n_T}](https://tex.z-dn.net/?f=X_i%3D%5Cfrac%7Bn_i%7D%7Bn_T%7D)
So,
![p_i=\frac{n_i}{n_T}\times p_T](https://tex.z-dn.net/?f=p_i%3D%5Cfrac%7Bn_i%7D%7Bn_T%7D%5Ctimes%20p_T)
where,
= partial pressure of gas
= mole fraction of gas
= total pressure of gas
= moles of gas
= total moles of gas
The balanced decomposition of ammonia reaction will be:
![2NH_3\rightarrow N_2+3H_2](https://tex.z-dn.net/?f=2NH_3%5Crightarrow%20N_2%2B3H_2)
Now we have to determine the partial pressure of
and ![H_2](https://tex.z-dn.net/?f=H_2)
![p_{N_2}=\frac{n_{N_2}}{n_T}\times p_T](https://tex.z-dn.net/?f=p_%7BN_2%7D%3D%5Cfrac%7Bn_%7BN_2%7D%7D%7Bn_T%7D%5Ctimes%20p_T)
Given:
![n_{N_2}=1\\\\n_{H_2}=3\\\\n_{T}=4\\\\p_T=866mmHg](https://tex.z-dn.net/?f=n_%7BN_2%7D%3D1%5C%5C%5C%5Cn_%7BH_2%7D%3D3%5C%5C%5C%5Cn_%7BT%7D%3D4%5C%5C%5C%5Cp_T%3D866mmHg)
![p_{N_2}=\frac{1}{4}\times (866mmHg)=216.5mmHg](https://tex.z-dn.net/?f=p_%7BN_2%7D%3D%5Cfrac%7B1%7D%7B4%7D%5Ctimes%20%28866mmHg%29%3D216.5mmHg)
and,
![p_{H_2}=\frac{n_{H_2}}{n_T}\times p_T](https://tex.z-dn.net/?f=p_%7BH_2%7D%3D%5Cfrac%7Bn_%7BH_2%7D%7D%7Bn_T%7D%5Ctimes%20p_T)
Given:
![n_{H_2}=1\\\\n_{H_2}=3\\\\n_{T}=4\\\\p_T=866mmHg](https://tex.z-dn.net/?f=n_%7BH_2%7D%3D1%5C%5C%5C%5Cn_%7BH_2%7D%3D3%5C%5C%5C%5Cn_%7BT%7D%3D4%5C%5C%5C%5Cp_T%3D866mmHg)
![p_{H_2}=\frac{3}{4}\times (866mmHg)=649.5mmHg](https://tex.z-dn.net/?f=p_%7BH_2%7D%3D%5Cfrac%7B3%7D%7B4%7D%5Ctimes%20%28866mmHg%29%3D649.5mmHg)
Thus, the partial pressure of
and
is, 216.5 mmHg and 649.5 mmHg