Calculate the pH. 0.5 M H3PO4

Q: How many grams of hNO3 must be dissolved to make 25 L of solution that has a ph of 1.5?

A: HNO3 is strong acid. Calculate the concentration of H+ ions,              pH = - log[H+][H+] =…

Q: Find the pH of a 0.010 M HNO2 solution.

A: HNO2 is a weak acid with dissociation constant, Ka = 7.2 X 10-4  Hence HNO2 will dissociate…

Q: What is the pH of a 0.0060 M KOH solution? A) 5.12 B) 2.22 C) 11.78 D) 8.88

A: The quantity capable of predicting solutions' acidic nature is named as pH. It can be related with…

Q: Determine the pH of the following solutions, using the information provided a) 1.25 ×10–3 M HNO3…

A:

Q: Calculate the pH of the following strong acid solution: 1.52 g of HNO, dissolved in 575 mL of…

A: Given:  Mass of HNO3 = 1.52 gm  Volume of solution = 575 ml  Molar mass of HNO3 = 63 g/mol

Q: What is the pH of a solution that has an [H+]=0.0470 M ? 3.06 12.7 1.33 8.42

A: We have to calculate the pH of Solution.

Q: Calculate the pH of a 0.015 M solution HBr .

A: Strong acid:The solution that is completely dissociates into its ions in water. This makes to…

Q: What is the pH of a 3.21 ×10 -2 M solution of KOH?   1.49 9.97 12.5 6.97

A: Given, Concentration of the KOH solution = 3.21 ×10 -2 M  pH of a 3.21 ×10 -2 M solution of KOH = ?…

Q: Calculate [H3O+] for a solution with a pH of 4.80.

A: We know that pH of solution = -log[H+] or…

Q: Calculate the pH of a 0.87 M methylamine solution.

A: pH of solution is defined as negative logarithm of hydrogen ions.

Q: Find the pH of a 0.0100 M sulfuric acid (H2SO4) solution

A: Given: Sulphuric acid (strong acid) Given acid is strong acid hence it completely dissociates into…

Q: What is the pH of a 0.00100M

A: Negative logarithm of H+ is called pH, to know the acidity of dilute solutions pH is introduced. pH…

Q: Calculate the pH of a solution that has [H301 = 3.1 × 10-8 M. A) pH 3.18 B) pH = 3.10 C) pH 7.51 pH…

A: Answer

Q: Calculate the pH of 0.024 M chloric acid

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Q: Calculate the pH of an a. 3.00 b. 4.00 с. 5.00 d. 6.00

A: Given, Ka = 4.9 x 10-10  PH = ?

Q: What is the pH of a 0.011 M HCIO4? **Report your answer to two decimal places. DO NOT worry about…

A: The name of the given acid is perchloric acid with chemical formula HClO4. It is a strong acid and…

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

A:

Q: 1) Calculate the pH of a solution with a hydrogen ion concentration of 4.5×106 M. a. Calculate the…

A: 1) Given, The concentration of the hydrogen ion = 4.5 × 10-6 M. pH of the solution = ? The formula…

Q: Calculate the pH of a solution that is 0.0400 M in *(a) H,PO4.

A: Answer  H3PO4 is weak acid       PH   = 1/2 [ Pka  - log c]…

Q: Calculate The PH Of 0.10M Na2C2O4

A: pH is a measure of acidity or basicity of a solution. A solution with pH less than 7 is considered…

Q: e Calculate the pH of a 0.24M sodium formate solution (HCOONA).

A: Given : concentration of HCOONa solution = 0.24 M  To calculate : pH of solution

Q: 6.)Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.

A:

Q: Find the pH of a 0.72M hydrochloric acid solution

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Q: What is the pH of a 5 x 10^-3 M KBr solution? Show all calculations.

A: KBr is a salt of strong acid (HBr) and strong base (NaOH)).  So it is a neutral salt.

Q: Calculate the pH of a 0.0644 M anilinium chloride solution. pH= Calculate the concentrations of…

A: Let us consider a ICE table below, HA = conjugate acid = 0.0644 M (anilinium chloride ) A- =…

Q: Calculate the pH of a 0.0750 M NH3 solution.

A: Since it is basic solution of NH3 so pH will be greater than 7.

Q: Calculate the pH of the following solutions.  - 0.10 M pyridine

A:

Q: 2. Calculate the pH of each of the following solutions: А. 0.0010 М НCІ В. О.76 М КОН C. A solution…

A: Following are the pH of the given solutions.

Q: Calculate [H3O+] for a solution with a pH of 8.37.

A: The given data contains, pH =8.37

Q: Calculate the pH of a 0.10 M NaBrO solution. (a) 3.22 (b) 10.78 (c) 11.02 (d) 9.96

A: NaBrO is a salt of strong base NaOH and weak acid HBrO. The pH can be calculated using the following…

Q: Hydrazine, N2H4 has Kb= 1.3E-6. Calculate the pH of 0.486M solution of N2H4.

A: Hydrazine is a weak base.We have to calculate pH given hydrazine solution. Recall the following…

Q: A 0.0059 M solution of H2SO4 would have a pH of... (choose the best answer) * 3.8 .0118 O 1.9 0.0059

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Q: Calculate the pH of a solution that is 0.0400 M in "(a) H,PO4. (Ь) Н.С.О. "(c) H,PO3.

A:

Q: Determine the pH of a solution with [OH"] = 6.83 × 103 M. Your answer should contain 3 decimal…

A: pH is the negetive logarithmic value of the concentration of H+. That is, pH = -log[H+]

Q: Calculate the pH for 0.43 M NH4ClO4

A: pH can be calculated by following formula  pH = - log [H+]

Q: 8) Determine the pH of the following solutions: a) 0.20 М СHСООН

A: The answer for part a) is given below. Kindly post the other subpart as separate question

Q: 4. Calculate the pH of a 0.92M hydrosulfuric acid solution.

A: Ph of diprotic acid is double the concentration of the acid as on dissociation it will give 2 H+…

Q: Calculate the pH of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10-5) HC2H302 - H* + C2H3O2…

A: pH measures the strength of acids and base that how the solution is acidic and basic lower the pH…

Q: Calculate the pH of a 0.55 M solution.

A:

Q: culate the pH of a solution that is 0.0853 M LiNO2 at 25

A: Given : Molarity of LiNO2 = 0.0853M

Q: What is the pH of a 0.025 M pyridine solution? (Kb value for pyridine = 1.7x 109)

A:

Q: Calculate the pH of the following aqueous solution:           0.62 M H2S (pKa1 = 7.00; pKa2 =…

A: H2Saq⥪H+aq+HS-aq                                       pKai=7.00                PKa1=-log Ka1…

Q: Calculate the pH of a 1.77 M NH4CN solution.

A: An acid is a substance that gives  ions in its solution whereas a basic substance gives  ions in its…

Q: Question attached

A: pH of any solution is measure the their acidity or basicity  it can be calculate as following…

Q: What is the pH of a 0.200 M solution of HNO3?   0.70   1.31   6.18   8.53

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Q: 1. Calculate the pH of the following: a. [H*] = 1 x 10³ M %3D b. [OH]=1 x 10$ M C. [H]=1 x 107 M

A: Calculate pH of the given data---

Q: The pH of a solution is 5.93. Find the pOH, [H;O*], and [OH-].

A:

Q: Calculate the pH of a 0.56 M benzoic acid solution.

A:

Q: Determine the pH of 1.5 M HBrO. (Ka HBrO = 2.5 x 10–9)

A:

Q: Calculate the number of hydronium ions

A:

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.