Calculate the pH of a 0.030M LiOH solution. Show all work below

Q: Calculate the hydrogen concentration of a solution with pH =9 A. -9.54 B. -Not enough information…

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Q: What is the pH of a 0.475 M solution of diethylamine. Show your work and include any relevant…

A: Note: Hey there! Thank you for posting the question. Since the Kb of diethylamine is not given, we…

Q: Rank the acids in the table below from strongest (1) to weakest (4). The most acidic H atom in each…

A: Acid is the substance which donate the proton .  The substance which lose the Proton easily is…

Q: 4. Determine the pOH given the following values: a. [H] = 2 x 10-8 b. [OH-] = 5.1 × 10-11

A: In this question we have to tell the POH of the given solution.

Q: Find the pH of 0.25M KF. Given Ka (HF) = 6.9x10-4 Show all work, use an ICE table and equation.

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Q: Find the pH and pOH of 0.010M HBrO4 solution. Show all your work.

A: Given, Concentration of HBrO4 = 0.010 M PH is defined as negative logarithm of concentration of…

Q: Using the Kb from the previous question, what is the pH of an 0.0100 M solution of sodium benzoate.…

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Q: Calculate the pH of a 0.42 M H,SO4 solution. Give your answer to 2 places after the decimal.

A: given, molarity of H2SO4 solution = 0.42 M

Q: Which of the following will be the weakest acid? А) HBro B) HBRO2 C) HBRO: D) HBRO4

A: The strength of an acid depends on the stability of the anion formed after the loss of proton.More…

Q: Please help with the last 3 part (18,19,20). Explain. Thanks

A: Enantiomers : These are the isomers having same structural formula but their mirror images are non…

Q: Given the ff data: 1.00 mL≎ 1.117 mL HCl, the HCl is 0.4876 N. How much water should be added to 100…

A: Answer: Product of normality and volume of solution is always equal to the gram equivalents of the…

Q: 9. Calculate the pH corresponding to each of the concentrations given below, and indicate whether…

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Q: 1) Determine the ArH° for the following reaction:

A: the standard Enthalpy of reaction is calculated by the following formula, ⊿r H0=sum of standared…

Q: Calculate both H3O* | and [OH] for a solution for which pH = 1.38. Enter your answers in scientific…

A: i.e. [H3O+] = 4.16*10-2 M

Q: Which is the strongest acid? HO. CI HO. F HO. HO. Br

A: Acids are those substances that  donate H+ ions in the solution. If any group present in the…

Q: Calculate the [H+] and pOH of a 0.0005 M solution of Boric acid. Ka=5.90x0^-10​

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Q: Construct the expression for Ka for the weak acid, HC,H,04. HC,H,0,(aq) + H,0(1) = H,0*(aq) +…

A: Given, given chemical reaction as follows,HC9H7O4(aq)+H2O(l)⇌H3O+(aq)+C9H7O4-(aq)we are asked to…

Q: Which one of the following solutions is basic?  a. A solution for which [OH-] = 8.3x10-12  M  b.…

A: We know that, pH is greater than 7, then solution is basic. So,

Q: Calculate the pH of a 0.083 M solution of HClO,. Report your answer to two decimal places.

A: HClO4 is a strong acid, it gives H+  ions in aqueous solution. pH of a solution is determined from…

Q: Use the References to access important values if needed for this question. What is the pH of an…

A: The pH of a solution refers to the measure of the molar concentration of the H+ ions that are…

Q: Must Show All Work For Full Credit!!! Find the pH, pOH, and the [OH] of a 3.25 x 104 M H2SO4. Hint…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: H H. H H H. нн (Choose one) (Choose one) (Choose one) (Choose one)

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Q: **Show your work where necessary. Example given in red! [H] pH [OH] pOH Acidic/Basic/Neutal? 1x…

A: According to question,Given,pH + pOH = 14 “Since you have posted a question with multiple sub-parts,…

Q: Which of the following represents the most acidic solution? How do you know? Explain in a separate…

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Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kb of NH= 1.8 x 105) NH4* + H2O+…

A: In the given question we have to calculate the pH of 0.6 M NH4Cl Solution. we know that the ammonium…

Q: MOST ACIDIC. Lon HO, HO. OMe NME2 A B C E Enter your answer here

A: Acidity is defined as the ease with which a molecule can donate protons. if it can donate PROTONS…

Q: Calculate the pOH of a solution  with [OH-]  = 4.5x 10 -14 M

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Q: Calculate the pOH of a solution with [H+]= 1.4 x 10^-9 M.

A: Given: [H+]= 1.4 x 10-9 M

Q: Calculate [H+] for each solution.

A: pH = -log [H+] [H+] = antilog pH [H+] = antilog(5)  [H+]  = 10-5 M

Q: What is the pH of 0.6 M NH4Cl solution? Discuss your results. (Kb of NH= 1.8 x 10-5) NH4++ H2O↔…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

Q: Show your work for the question above: "12. What is the pH of a solution in which [OH] = 0.000005…

A: Given in the question , [OH-1] = 0.000005 m pH = 14 + log[OH-1]

Q: Use: pH = -Log [H30*] 1. Round answers to the tenths place: (show work) a) Find the pH of a solution…

A: pH: It is defined by saying that power of hydronium ions, on the basis of this w can categorize the…

Q: For the acid HA (where Ka >> 1), what is the pOH at 25o C if the initial HA concentration is 0.047…

A: Given:  concentration of HA = 0.047 M  To find: pOH = ?

Q: What is the pH of a solution that has a [OH-] of 8.5 x 10-4 please show work

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Q: Calculate the pOH of 1.5 x 10⁻⁷ M HCl solution.

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Q: pH and pOH of [H+] = 4.02×10-8 M

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Q: that

A: We know that a bunsen burner is made for Laboratory use. It consists of a barrel, collar, air holes,…

Q: Could someone please explain how to answer this question and show work for the calculations to…

A: Orange and green colors when get mixed give the color brown.

Q: place the following in order of increasing acid strength. HBrO2, HBrO3, HBrO, HBrO4

A: Arrange the following in order of their increasing acidic strength : HBrO2, HBrO3, HBrO,  HBrO4 .

Q: List the following bases in order of strength, strongest to weakest. O NH4OH, Kb=1.8x10-3 O NH3,…

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Q: Calculate the values of [OH-] , and PH from Kb and [B initial]. Calculate the values of [OH-], POH…

A: NH3 dissociates as:                              NH3  +  H2O  ⇋  NH4+ +  OH-Initial mol…

Q: The pOH of a solution is 9. Which of the following is correct? (A) The solution is basic with an…

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Q: A 0.25 M solution of a weak acid has a measured pH = 2.55. On a separate piece of paper, determine…

A: Since you have posted multiple unrelated questions, we are entitled to answer the first only.

Q: Consider three generic acids: HX, HY, and HZ. 58 -11 HX ⒸH* ox Arrange the acids according to…

A: Strong acids dissociate completely into ions in the aqueous solution. Weak acids partially…

Q: calculate the pOH of [H=] = 2.5 x 10-5 m a. 9.40 b. 4.0 x10^-10 c. none  d. 14.0 e. 4.60

A: Given is, [H+] = 2.5 x 10-5 M

Q: Calculate theoretical pH for each solution recorded in Data Table 1. Remember for weak acids (and…

A: pH is defined as negative logarithm of concentration of hydrogen ions. pH = - log[H+] Similarly, pOH…

Q: If a solution has a hydroxide ion concentration of 1x10-10, the pH of the solution is? Show work.

A: Given, [OH-] = 1 x 10-10 We know, PH = -log [H+] POH = -[logOH-] POH = - log [1 x10-1] POH = - (log…

Q: Calculate the pOH of the following solutions at 25°C. (a) [OH]-8.47 x 10-11 %3D РОН %3D (b) [OH ]=…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.