MBA6320_HW1_Edwards

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Which of the following is true  about pH probe? a. A pH probe consists of a metallic indicator. b. A pH probe will always have an SCE reference electrode. c. A pH probe is specific for measuring proton concentrations. d. A pH probe is an ion selective electrode that consists of a concentration cell.

Instead of using an electrode to collect ions, why electron multiplier is needed as the detector for MS?

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Calcium in a 100.0 mL sample of fuit juice was analyzed by an electrochemical method that gave a detector current of 2.40 mA. A standard addition of 10.00 mL of 80.0mg/mL calcium ion increased the current to 4.56 mA. Find the concentration of calcium in the fruit juice.

Táke off any gridlines and add a title and axes labels. Add the trendline and the relevant equation. b) If a sample was analyzed and the current was measured to be 5.18 mA, what is the concentration of analyte in the sample? 5.18= 3.403x + 1.9232 3.2368=3.4403 x 0.947: x Pentane (C5H12) is a liquid with density of 0.929 g/mL at 25 °C. Find the true mass of pentane when the mass in air is 14.82 g. Assume air density is 0.0012 g/mL.

If a pH electrode is experiencing the sodium (alkaline) error... A. the apparent pH will be lower than the true pH. B. the apparent pH will be higher than the true pH C. there will be no effect on the pH, but the glass membrane will dry out because of the sodium. ●

21. (What exactly is meant by potentiometric methods? What are they even?)

Analytical Chemistry II Why is carbon used as an electrode in arc and spark sources? Explain briefly

complete: reference electrode is N O T ___   i . i n   c o n s t a n t   p o t e n t I a l ii. r e s p o n d I n g   t o   a na l y t e   c o n c e n t r at I o n iii.  g i v i n g   s t a bl e   r e s p o n s  e

calculate the [FESCN2+] using volumes of stock solutions. Presume that all of the SCN- ions react. Next, record the light absorbance values of each standard solution. Volume Volume Volume [FESCN2+] Absorbance Standard Fe(NO3)3 SCN- H2O sample (mL) (mL) (mL) 1 2.50 2.00 20.50 0.1811 2 2.50 1.50 21.00 0.3219 2.50 1.00 21.50 0.4981 4 2.50 0.50 22.00 0.6328 Stock [Fe(NO3)3] = 0.200 M, Stock [SCN-] = 0.0020 M. %3D

The basic setups for electrochemical measurement include all of the following, EXCEPT: Group of answer choices   A. Measure the potential while controlling the current. B. Measure the current while controlling the potential. C. Measure the potential at zero current. D. Measure the potential and current simultaneously.

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Calculate the molarity of prepared solution?

Ascorbic acid (vitamin C) in a 50.0-mL sample of orange juice was analyzed by an electrochemical method that gave a detector current of 1.78 mA. A standard addition of 0.400 mL of 0.279 M ascorbic acid increased the current to 3.35 mA. Find the concentration of ascorbic acid in the orange juice.

Match each commercial application of electrochemistry with the appropriate description.   a.     electroplating b.     secondary cell c.     cathodic protection d.     electrorefining e.     fuel cell f.      Hall-Heroult process g.     dry alkaline battery     ____ 1. measures taken to prevent corrosion     ____ 2. a battery where the reactants are continuously replenished     ____ 3. a primary cell       ____ 4. the application of a thin coating of a metal that resists corrosion     ____ 5. the use of molten cryolite to produce aluminum     ____ 6. a rechargeable battery     ____ 7. the process used to obtain high-grade, pure metals from impure materials

Which statement is NOT correct?     pH meter should always be standardized before using to make sure that your readings are accurate and repeatable.     The electrode tips should never touch the bottom or sides of a beaker.     When finished using the pH meter, rinse the electrode and place it in the pH 7 buffer solution on standby.     One buffer solution is enough to standardize a pH meter before using.

One electrochemical technique involves first depositing an analyte on the surface of an electrode, then using an applied current to remove the analyte via a reduction or oxidation reaction. What is this method called? A. Cyclic voltammetry B. Polarography C. Amperometry D. Hydrodynamic voltammetry E. Stripping voltammetry

11. Undercharging has high adverse impact on a. AGM Battery c. Gel battery 12. A relative measure of cell electrical current a. Columbic efficiency c. Life time b. Lead Carbon battery d. Air-Metal Battery b. C-Rate d. Power density

If we had potassium vapor lamps, what color would they be?

22.a. Which of the following statements describes the change of specific gravity during battery charging?A. The specific gravity increases faster than the state of charge.B. The specific gravity lags behind the state of charge.C. The change in specific gravity with time is directly proportional to the amount of charge.D. A hydrometer reading shows the true state of charge when taken shortly after charging has begun.22.b. The purpose of the vent on the top of a lead-acid cell is toA. permit the gas to escape during charging.B. add water to the cells.C. trap the hydrogen gas generated during charging.D. remove the sediment developed during charging.

Uses of Substances based on their Chemical Bonds Objective: To discover the uses of some substances based on their chemical bonds. I. I. Materials: Flashlight bulb 3V -battery Connecting wires (exposed ends) Metal strips of aluminum, copper, iron Distilled water NaCI Small Beaker II. Procedure: 1. To show the conductivity of table salt, NaCl, prepare a simple circuit consisting of a flashlight bulb, 3V- battery, and connecting wires with insulator ends removed. Prepare 200 cc of distilled water in a small beaker and immersed the ends of the connecting wire in the water as shown below. Observe the bulb if it would light. Mix 5 g of NaCl in the distilled water and observe the bulb. Did it light? electrodes wire saltwater battery light bulb 2. Add 5 g more, mix and observe the bulb again. 3. Repeat procedure 2. 4. To illustrate the electrical conductivity of different metals, prepare strips of aluminum, copper and iron. Use the circuit in procedure 1. Connect the bare ends of the wire to…

1. Identify the components of a pH electrode and explain their functions. Explain throughly.

DOL The Chemistry of Rusting-An Introduction to Unit 4: Chemical T Flaking Away - Check Your Understanding For each question, answer on your own in the first row of the table. During partner time, share your responses and revise your answers as needed, recording them in the second row. Be prepared to share during the whole-class discussion. Record final your answer to each question in the last row of the table. 1. Write a short paragraph that connects the following words: oxidation, reduction, anode, cathode, and electrons. My first answer, thinking on my own: My revised answer after discussing it with my partner: My final answer after the whole-class discussion: НА

The standard hydrogen electrode (SHE) is used as a reference electrode. True or  false?

A Ni half-cell was coupled to a Ti half-cell to form a cell at equilibrium conditions: a. Plot and identify ZA and ZC zones, current and electron flow. b. Potential difference between half cells. c. What is the energy generated by the system. Data: Standard potential Vs ENH: Ti= 1200 mV and Sn= -136 mV. The density of Ti = 4.51 g/cm3 and Ni = 8.9 g/cm3. Consider unit areas 1 cm2

1. IOn selective electrode utilizing pCO2 is used fro the measurement of the electrolyte    a. Phoisphate  b. bicarbonate  c. Magnesium  d. chloride  e. sodium    2.  The confirmatory method for the measurement of Calcium and Magnesium  A. Turbidimetry  b. FES  c. none  d. colorimtery  e. AAS    3. the electrolyte is found as component of phospholipids, nucleic acids, creative phosphate and ATP a. magnesium  b. calcium  c. phosphate  d. bicarbonate  e. chloride

How does hydronium ion concentation relate to electrode potential in potentiometry? a. As temperature increases, the pH also increases. b. Each pH unit represents a 59.1 mV change in potential. c. The increase in pH is linear relationship to the electrode potential. d. Decreased H+ concentration is directly proportional to electrode potential. e. none of these

Which form if EDTA is used in any analytical experiment? Why?

Explain the function of each electrode in the polarography cell

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