The main formulas are <span>pH=pKa + log(Base/Acid) and pKa = </span><span>-log(Ka)
so firstly, we must find the value of pKa,
Ka=6.37 x 10 ^-5, and then logKa= log (6.37 . 10^-5)= -9.66, so -logKa= +9.66=Ka
next let's find </span><span>log(Base/Acid)
for that the concentration of NaOH is [NaOH] = </span><span>500.0 x 0.110 / 500+535 =0.053M, the concentration of the Acid is [Acid] =535*0.25 / </span><span>500+535 =0.12M, so its difference is </span><span><span>[Acid]-</span>[NaOH] = 0.12-0.053=0.07
so pH=</span><span><span>pKa + log(Base/Acid)= 9.66 + log(0.053 / 0.07)= 9.66-0.36=9.29</span> </span>
so pH=9.29.
Answer:
Liquid A is a homogeneous mixture and Liquid B is a heterogeneous mixture
Explanation:
Answer:
7.32g of HNO3 are required.
Explanation:
1st) From the balanced reaction we know that 2 moles of HNO3 react with 1 mole of Ca(OH)2 to produce 2 moles of H2O and 1 mole of Ca(NO3)2.
From this, we find that the relation between HNO3 and Ca(OH)2 is that 2 moles of HNO3 react with 1 mole of Ca(OH)2.
2nd) This is the order of the relations that we have to use in the equation to calculate the grams of nitric acid:
• starting with the 4.30 grams of Ca(OH)2.
,
• using the molar mass of Ca(OH)2 (74g/mol).
,
• relation of the 2 moles of HNO3 that react with 1 mole of Ca(OH)2 .
,
• using the molar mass of HNO3 (63.02g/mol).

So, 7.32g of HNO3 are required.