Answer:
A) [H3PO4] will increase, [KH2PO4] will decrease, and pH will slightly decrease.
Explanation:
A buffer is a solution which resists changes to its pH when a small amount of acid or base is added to it.
Buffers consist of a weak acid (HA) and its conjugate base (A–) or a weak base and its conjugate acid. Weak acids and bases do not completely dissociate in water, and instead exist in solution as an equilibrium of dissociated and undissociated species. When a small quantity of a strong acid is added to a buffer solution, the conjugate base, A-, reacts with the hydrogen ions from the added acid to form the weak acid and a salt thereby removing the extra hydrogen ions from the solution and keeping the pH of the solution fairly constant. On the other hand, if a small quantity of a strong base is added to the buffer solution, the weak acid dissociates further to release hydrogen ions which then react with the hydroxide ions of the added base to form water and the conjugate base.
For example, if a small amount of strong acid is added to a buffer solution that is 0.700 M H3PO4 and 0.700 M KH2PO4, the following reaction is obtained:
KH₂PO₄ + H+ ----> K+ + H₃PO₄
Therefore, [H₃PO₄] will increase, [KH₂PO₄] will decrease, and pH will slightly decrease.:
Answer : The enthalpy change for the process is 52.5 kJ/mole.
Explanation :
Heat released by the reaction = Heat absorbed by the calorimeter + Heat absorbed by the solution
![q=[q_1+q_2]](https://tex.z-dn.net/?f=q%3D%5Bq_1%2Bq_2%5D)
![q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]](https://tex.z-dn.net/?f=q%3D%5Bc_1%5Ctimes%20%5CDelta%20T%2Bm_2%5Ctimes%20c_2%5Ctimes%20%5CDelta%20T%5D)
where,
q = heat released by the reaction
= heat absorbed by the calorimeter
= heat absorbed by the solution
= specific heat of calorimeter = 
= specific heat of water = 
= mass of water or solution = 
= change in temperature = 
Now put all the given values in the above formula, we get:
![q=[(12.1J/^oC\times 6.1^oC)+(100.0g\times 4.18J/g^oC\times 6.1^oC)]](https://tex.z-dn.net/?f=q%3D%5B%2812.1J%2F%5EoC%5Ctimes%206.1%5EoC%29%2B%28100.0g%5Ctimes%204.18J%2Fg%5EoC%5Ctimes%206.1%5EoC%29%5D)
Now we have to calculate the enthalpy change for the process.
where,
= enthalpy change = ?
q = heat released = 2626.61 J
n = number of moles of copper sulfate used = 
Therefore, the enthalpy change for the process is 52.5 kJ/mole.
Here you are! I hope it helps, and also for the ones I put a red ‘x’ it depends on how you round it.
The question is asking to state the substance that is acting as the Bronsted Lowry base in the forward reaction, base on my research, I would say that the substance acting to said formulas is the NH3. I hope you are satisfied with my answer and feel free to ask for more if you have question and further clarification
Yes they break down what they are made of and figure it out.
