Suppose you have a solution of 0.1 M H2CO3 and 0.1 M NaHCO3. Which of the following reactions takes place with addition of small amount of NAOH to this buffer solution? O H* + HCO3 -->H2CO3 O OH + HCO3 --> H20 + CO32- none of the choices
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- Suppose you have a solution of 0.1 M H2CO3 and 0.1 M NaHCO3. Which of the following reactions takes place with addition of small amount of NaOH to this buffer solution? O H* + HCO3 -->H2CO3 O none of the choices O OH + HCO3 - -> H2O + CO3²- O OH + H* --> H2OIn the following reaction in aqueous solution, the acid reactant is and its conjugate base product is CH;COOH + NH3 CH;CO0 + NH,"Assuming ideal behavior, rank the solutions boiling points, 1 is lowest to 4 highest boiling point: 0.1 m CaCl2 0.1 m NaOH [Choose ] [Choose ] 0.025 m Al2(SO4)3 [Choose] 0.25 m C6H12O6 [Choose ]
- Please balance the following half-based reactions: SbH3 → Sb (acidic solution) BrO3- → Br2 (acidic solution) Cl- → ClO2- (basic solution) (PLEASE DONT USE H+ ION INSTEAD SUB H30+ )Balance each of the following redox reactions occurring in acidic solution. Part A VO2 (aq) +ClO2 (aq) →VO2+(aq) + ClO2(g) Express your answer as a chemical equation. Identify all of the phases in your answer. = ΑΣΦ ? A chemical reaction does not occur for this question. You have already submitted this answer. Enter a new answer. No credit lost. Try again.What volume of 0.1M NaOH (reagent) needs to be added to increase your 7.5 pH (buffer) by 0.5 pH units. The goal is to further purify MOPs (see image). Protonated form = 6.6 x 10.3^-3 mol/L Deprotonated form = 1.32 x 10^-2 mol/L Show calculations.
- The following exothermic reaction is at 0.00 °C and 1.00 atm SeO4 (g) ⇌ Se(g) + O2(g) , kc = 2.4 ×10-6 The reaction contains [SeO4] = 0.100 M, [Se] = 0.0034 M, [O2] = 0.0022 M Does the reaction exist at equilibrium? If not, in what direction it will proceed? Question 22 options:Acetic acid is the principal ingredient in vinegar as shown; that's why it tastes sour. At equilibrium, a solution contains [CH3CO2H] = 0.0787 M and [H3 O+] = [CH3 CO2−] = 0.00118 M. What is the value of Ka for acetic acid?Nitrogen and hydrogen react to form ammonia, like this: N2(g)+3H,(g) → 2 NH,(g) Imagine 56. mmol of NH, are added to an empty flask, and then answer the following questions. O Zero. What is the rate of the reverse reaction before any NH3 has been O Greater than zero, but less than the rate of the forward reaction. added to the flask? Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse reaction just after the NH, has been added to the flask? O Greater than zero, but less than the rate of the forward reaction. Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. O Zero. Greater than zero, but less than the rate of the forward reaction. What is the rate of the reverse reaction at equilibrium? Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and…
- A patient presents to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 4.0×10-4 M and bicarbonate ion (HCO3-) 3.062×10-3 M. Ka = 4.3 × 10-7 H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?Suppose you wanted to make a buffer of exactly pH 7.00 using KH2PO4 and Na2HPO4. If the final solution was 0.1 M in KH2PO4, what concentration of Na2HPO4 would you need?A researcher wants to look for glucaronic acid conjugated metabolites in sample of urine(glucaronic acid conjugation is a common method of metabolism for excretion.) Pronotated glucaronic acid conjugated metabolite ions often lose anhydroglucaronic acid(176 Da) during low energy CID. Which triple quadrupole experiment might be best for finding these conjugates?
