Post Lab 2 Inorganic Lab

PLEASE PLACE THE ANSWERS IN A SQUARE BOXES SAME AS THE QUESTION. SO I COULD KNOW WHICH ANSWERS BELONGS TO THE RIGHT PLACE.

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

Draw a structure for the product of the acid-base reaction below. t H3C CH3 . Include all valence lone pairs in your answer. • If the reaction is a Lewis acid-base reaction, draw the products in a single sketcher, with a single bond connecting the Lewis base and Lewis acid. • If the reaction is a Brønsted acid-base reaction, draw the products in separate sketchers. • Include all nonzero formal charges. 3 TI +▾ + AICI 3 *9-85 CH To Q Q 4 [F Previous

Draw a structure for the product of the acid-base reaction below. Include all valence lone pairs in your answer. If the reaction is a Lewis acid-base reaction, draw the products in a single sketcher, with a single bond connecting the Lewis base and Lewis acid. If the reaction is a Brønsted acid-base reaction, draw the products in separate sketchers. Include all nonzero formal charges.

I need help with this question. Can you help me to show the work like step by step

please answer ASAP

Consider the Lewis structure for hydrogen fluoride (HF). H—F : A. If hydrogen fluoride were to behave as an acid (assuming that was possible), draw and upload as an attachment here the Lewis structure of its resulting conjugate base. B. Reflecting on your answer for Part A and using the three acid-base models from Q1, would you predict the conjugate base would form? (Does this situation make sense)?

In CHEM 160, you learned that AgBr does not dissolve in water.  Why is that?  (Choose the best answer.) Group of answer choices A:It is possible to separate the Ag+ and Br- ions in water under reasonable conditions but this step requires more energy than what is released by the solvation of these ions by H2O molecules. B:We lied in CHEM 160 - AgBr is actually very soluble in water. C:It is possible to separate the Ag+ and Br- ions in water under reasonable conditions and this step requires less energy than what is released by the solvation of these ions by H2O molecules. D:Separating the Ag+ and Br- ions to an appreciable extent in water requires to much energy to accomplish under reasonable conditions. Consider this picture depicting the hydration of an atom or ion by water molecules.  Of the choices below, what is the only atom or ion that the yellow particle in the center can be?   Group of answer choices A:K+ ion B:oxygen atom in ethanol (CH3CH2OH) C:Cl-…

[Review Topics] [References] Use the References to access important values if needed for this question. Identify whether each species functions as a Brønsted- Lowry acid or a Brønsted-Lowry base in this net ionic equation. H₂PO4 + H₂S (aq) Brønsted- Brønsted- Lowry Lowry = - H3PO4 (aq) + In this reaction: The formula for the conjugate H₂PO4 is Submit Answer The formula for the conjugate is Brønsted- Lowry Retry Entire Group of ✓of H₂S 7 F10 HS™ Brønsted- wry F11 ☐ F12 Up

3.

Please help me with this, double check your answers other tutors got it wrong.

5. Complete the table: Chemical System 1. 1 М КСI 2. 1 M H2SO4 3.1 М КОН 4. 1 M HE 5. 1 M AI(OH)3 6. 1 М НСI 7.1 M table sugar Type of Substance | Intensity of Light Classification Typeofsubstance- ionic, strongacid, strong base, weak acid, weak base, organic which is neither an acid norbase

a Draw a structure for the product of the acid-base reaction below. :o: BF3 + • Include all valence lone pairs in your answer. • If the reaction is a Lewis acid-base reaction, draw the products in a single sketcher, with a single bond connecting the Lewis base and Lewis acid. • If the reaction is a Brønsted acid-base reaction, draw the products in separate sketchers. • Include all nonzero formal charges.

6. please pick the correct option

‪I just need an answer. An explanation isn’t necessary. Thank you.‬

PLease help me find the right answer please be sure to express your answer in a chemical formula

b My Questions | bartleby rellum.ecollege.com/course.html?courseld%316519516&OpenVellumHMAC=Da14e8ada06537be6b0 Best Free PowerP... L Google Drive Academic Search I Downloads ouTube Maps Submit Request Answer Part G Write the formula of the conjugate acid for base Br. Express your answer as a chemical formula or an ion. NA chemical reaction does not occur for this question. Submit Request Answer Part H Write the name of the conjugate acid found in part G. Spell out the full name of the compound. Submit Request Answer

1. Consider Lewis structure for methane (CH4). a. If methane were to behave as an acid (if possible), draw the Lewis structure of its resulting conjugate base. b. Reflecting on your answer for Part A and using the three acid-base models above, would you predict the conjugate base would form? (Does this situtation make sense)? c. If methane were to behave as a base (if possible), draw the Lewis structure of its resulting conjugate acid. d. Reflecting on your answer for Part A and using the three acid-base models above, would you predict the conjugate acid would form? (Does this situtation make sense)?

Base simulation

True or false?

CH;COOH so,?- CH;COO HSO; Brønsted-Lowr Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry acid base In this reaction: The formula for the conjugate O of CH3COOH is The formula for the conjugate of SO,- is Submit Answer Retry Entire Group 9 more group attempts remaining Use the References to access important values if needed for this question. Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. HCIO co,²- CIO HCO; Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugat v e of HCIO is acid base The formula for the conjugate 8 of CO,2 is Use tne Keierences to access important values iI neeaea ior this question. Identify whether each species functions as a Brønsted-Lowry acid a Brønsted-Lowry base in this net ionic equation. HCIO H,S (aq) + HS CIO Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate 8 of HCIO is The formula…

Is the order of acidity correct? Why or why not?

Electrical Conductivity of solution lons released in solution Solution pH Taste 1 Very high 8.0 bitter ОН- 2 Very high 14.0 bitter ОН - none 7.0 none both 4 Very high 2.0 H+ sour Based on the experimental data collected by a student above, which solution is acidic? Give at least 2 reasons to support your answer.

‪I just need an answer. An explanation isn’t necessary. Thank you.‬

6.

Can you help me correcting this: I have  good the answer but  To justify the order of the number of oxygens with the same halogen, there is a trend associated with the oxidation number of the halogen - find that trend and cite it. Can you help me with this, please?

Can you please show me the computation or how to compute? Thank you.

Thank you!

. Suppose you have already compared the pH values of two substances using 0–14 paper. When would a follow-up test using 4.5 – 7.5 paper be most helpful?           When both substances had a pH value of about 3 on the 0 – 14 paper.         When both substances had a pH value of about 6 on the 0 – 14 paper.             When both substances had a pH value of about 9 on the 0 – 14 paper

What would be the conjugate base of HSO4- ? Express your answer as a chemical formula.