Answer:
- (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄)
Explanation:
A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid.
Also, a buffer solution is a solution which resists changes in pH when acid or alkali is added to it.
- (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄) when dissolved in 1 L H₂O will produce a buffer because NaH₂PO₄ is considered as weak acid while Na₂HPO₄ is its conjugate base. 2.
- (0.1 mol H₃O⁺ + 0.1 mol Cl⁻) is not a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid.
- (0.1 mol HCl + 0.1 mol NaoH) HCL is a strong acid and NaOH is a strong base so it will not form a buffer when dissolved in water.
- (0.1 mol H₃O⁺ + 0.1 OH⁻) is not a mixture of a weak acid and its conjugate base, or weak base and its conjugate acid
- (0.1 mol NaCl+ 0.1 mol KCl) NaCL and KCL are salts so it will not form a buffer when dissolved in water.
So the right choice is
- (0.1 mol NaH₂PO₄ + 0.1 mol Na₂HPO₄)
7 is the pancreas and 8 is i can’t see the other choices but for diabetes the glucose levels will be a lot higher
Answer: PH= 1.4
Explanation:
n(mole)= concentration(c)× volume(v)
n(HClO4) = 0.08 ×0.03
n(HClO4)= 0.0024 mole
n(Ba(OH)2) = 0.28 × 0.05
n(Ba(OH)2) = 0.014
2HClO4 + Ba(OH)2.....>Ba(ClO4)2 + 2H2O.
Hence, the limiting reagent is perchloric acid. According to the reaction:
0.0024 HClO4 req 1/2× 0.0024 of Ba(OH)2.
n(Ba(OH) reacted= 0.0012
Excess n(Ba(OH)2) = 0.014-0.0012
Excess n(Ba(OH)2) = 0.0128
Conc(Ba(OH)2) unreacted = 0.0128/.32 (vol. of mix is 32ml)
= 0.04M = [H+]
PH = -log[0.04] = 1.397
PH= 1.4
Some of the symptoms from swallowing hydrochloric acid:
<span><span>
</span></span><span><span>-Abdominal pain
</span>-Breathing difficulty due to swelling of throat
-Chest pain
-Drooling
-Fever
-Mouth pain
-Rapid drop in blood pressure
-Throat pain <span>
-Vomiting blood</span></span>
Answer: The temperature of the gas is 132.25K and -140.75°C
Explanation:
Given that:
Volume of helium gas (V) = 18.5L
Temperature of helium gas (T) = ?
Pressure (P) = 0.85 atm
Number of moles (n) = 1.45 moles
Molar gas constant (R) is a constant with a value of 0.082 atm L K-1 mol-1
Then, apply the formula for ideal gas equation
pV = nRT
0.85atm x 18.5L = 1.45 moles x 0.082 atm L K-1 mol-1 x T
15.725 atm•L = 0.1189 atm•L•K-1 x T
T = 15.725 atm•L / 0.1189 atm•L•K-1
T = 132.25K
Given that temperature in Kelvin is 132.25, convert it to Celsius by subtracting 273
So, T(in Celsius) = 132.25K - 273
= -140.75°C
Thus, the temperature of the gas is 132.25K and -140.75°C
