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Explain how atmospheric nitrogen dioxide (NO2) decreases the pH of water in clouds and rain. In your answer, include balanced chemical equations for reactions of NO2 with water.

When coal is burned, it produces ______  which combines with _______  to form _________, SO2. This SO2 then reacts with_______  , which_______  the pH of normal rainwater. This acidic rainwater is also called_______  . It is responsible for dissolving valuable________  nutrients, but also converts normally harmless________  compounds into very toxic varieties. Fill in the Blank!

Consider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10

2. Aspirin is absorbed into the blood through the cells lining the stomach and the small intestine. Absorption requires passage through the plasma membrane, the rate of which is determined by the polarity of the molecule: charged and extremely polar molecules pass slowly, whereas neutral and hydrophobic ones pass rapidly a. The pH inside the stomach is around 2.0 and the pH of the contents of the small intestine is about 6.0. Which of the following statements is correct: i. The small intestine has 3 times lower [H] than the stomach. ii. The small intestine has 4 times lower [H ] than the stomach iii. The small intestine has 3,000 times lower [H] than the stomach iv. The small intestine has 10,000 times lower [H] than the stomach. b. The pKa of aspirin is 3.5. Draw the predominant form of aspirin and its overall charge (-1,0 or +1) when it is in the stomach or in the small intestine: Small Intestine (pH= 6.0): Stomach (pH 2.0) Overall Charge: Overall Charge:

From the National Oceanic and Atmospheric Administration graph about ocean pH above, the following conclusions can be made A. As dissolved carbon dioxide increases, pH becomes more acidic B. As dissolved carbon dioxide increases, pH becomes more basic C. As pH becomes more acidic, dissolved carbon dioxide increases D. As pH becomes more basic, dissolved carbon dioxide decreases

When some amount of the strong acid is added to a solution of nitrous acid,__ Ka for nitrous acid will increase. Ka for nitrous acid will decrease. O The percent ionization of nitrous acid will remain unchanged. O The percent ionization of nitrous acid will increase. O The percent ionization of nitrous acid will decrease.

Organic molecules often have polar covalent bonds. How does this provide opportunities for chemical reactions to occur at a specific site in a molecule? How could competitive reactions be controlled by adjusting the acidity/basicity of the chemical system?

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H+] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.735, the hydrogen ion concentration is mol/L.

Cite cases of acid rain phenomenon in the Philippines and briefly explain the condition of affected areas or regions.

1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.

Phosphoric acid, H3PO4(aq),H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.150 M phosphoric acid solution. pKa1= 2.16         pKa2= 7.21         pKa3= 12.32 [H3PO4]= ? M [H2PO−4]= ? M [HPO2−4]= ? M [PO3−4]= ? M [H+]= ? M [OH−]= ? M pH=

Explain how the process of denitrification will lead to a reduction of seawater pH, justify your answer with the use of a chemical equation. Name any two bacteria that aid the process of denitrification.

Phosphoric acid, H3PO4(aq),H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.400 M phosphoric acid solution. pKa1: 2.167 pKa2: 7.21 pKa3: 12.32

Kindly prepare short note in following environment incident in c & d

B. STANDARDIZATION OF A CALCIUM HYDROXIDE SOLUTION Write a balanced chemical equation for the reaction of hydrochloric acid with calcium hydroxide. Includes of reactants and products. Equation: 2HCI + cacoH) cac12+2H20 Data and Results: Molarity of hydrochloric acid Volume of hydrochloric acid Initial buret reading Final buret reading Trial 1 0.025 20.9. 2020L Volume calcium hydroxide used Moles hydrochloric acid used Moles calcium hydroxide used Concentration of calcium hydroxide Average concentration of calcium hydroxide Calculations: Trial 2 1000 mL 1.00 mL 060299 1000mL 0.30mL 19.00 mL mL mL L L 0 moles moles moles moles M M M 0.01000LHC (0.051800/241) = 0.000518300 1LHCl 0.000518HC (100/600) -0.000259 mol.com 2001 H M=0.000250 mol-0.0259M 0.01000 Experiment 21-A Review of Basic Laboratory Techniques

PREDICT THE MAJOR OR NO R ACTION OH 1) KM NO4, OH, HEAT 2) HOt

Please answer all the questions !!!

contaminated e Review Constants Periodic Table The presence of SO₂ in the atmosphere and the sulfuric acid that it produces result in the phenomenon of rainwater is naturally acidic and generally has a pH value of about 5.6. The pH of acid rain is about 4. This acidity has affected many lakes in northern Europe, the northern United States, and Canada, reducing fish populations and affecting other parts of the ecological network within the lakes and surrounding forests. The pH of most natural waters containing living organisms is between 6.5 and 8.5, but freshwater pH values are far below 6.5 in many narts of the continental United States At nH levels helow 4.0 all vertebrates most invertebrates and many microorganisms are Part A If the pH of a 1.00-in. rainfall over 1600 miles² is 3.60, how many kilograms of sulfuric acid, H₂SO4. are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Kal is very large and K2 is 0.012. Express your answer to two…

Indicator of the acidity or the alkalinity of sewage/wastewater. pH Temperature Dissolved Oxygen Total Suspended Solids A measure of how much oxygen is consumed by bacteria or microbes as they break down organic pollutant in water. * COD BOD Dissolved Oxygen None of the above

Rainwater is naturally acidic due to the formation of carbonic acid from dissolved carbon dioxide (CO2)(CO2). Atmospheric sulfur oxides, produced when coal is burned for fuel, can cause rainwater to become even more acidic. In some locations, pH values below 5 have been measured. Results of the increasing acidity include increased ocean acidification, slowed coral growth, and damage to marble statues. Balance the equations related to the acidification of rain by inserting coefficients as needed. If the equation is already balanced, leave it as is. equation 1: S+O2⟶SO2S+O2⟶SO2   equation 2: SO2+O2⟶SO3

Name the two ways that remove the most carbon dioxide from the atmosphere.  Carbon dioxide combines with water to form a single product.  Name that product (label it as product #1).  That product #1 reacts with water to produce hydronium ion and product #2.  Name product #2.  BRIEFLY: How do these two reactions affect ocean pH?  BRIEFLY: how does ocean pH affect ocean-dwelling organisms?

A Dashboard 101 Chem101 + а ap.101edu.co Question 10 of 16 Submit Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH:(aq) + HCI(aq) - 14- O3- |2+ 3+ 14+ 1 2 3 4 7 9. 1 I5 16 (s) (g) (aq) H3O+ H2O OH- CI Reset • x H2O Delete + 10:24 PM P Type here to search 65°F Mostly sunny 10/31/2021 1L

Provide brief explanation about the chemistry principle and concept of the following reaction

Correlate human activities to the occurrence of acid rain

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

10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?

Which of the bases are strong bases and which are weak from Table 1? For the strong base,calculate the pH:

doug began preparing laboratory surface disinfectant from chlorine bleach. he put on a chemical resistant apron and gloves and then removed the bleach container from the special chemical cabinet. he carefully placed the container on the laboratory benchtop and began to add the chlorine bleach to distilled water. nearby workers began complaining of burning eyes. doug was reprimanded by the supervisor. Explain why.